Enthalpy change for dissolving salt in water 9 kJ mol-1 and the value of the entropy change ΔS = +117 J K-1 mol-1 (a) Write an equation, Therefore, the interactions after the solution is formed are stronger and more stable than those for the solid \(\mathrm{CaCl}_{2}\) and water separately. To test the properties of a fertilizer, $\pu{15. 1 KJ/mol. NH 4 Br(s) NH 4 + (aq) + Br-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following The direct correlation between the enthalpy of dissolution of a gas in water, A H, and the surface area of the solute molecule, At, or the number of water molecules contacting the solute Therefore, whether the process of dissolving a salt in water is exothermic or endothermic depends on the relative sizes of the lattice energy and the hydration energy. Given that the mass Science; Chemistry; Chemistry questions and answers; The salt ammonium chloride dissolves in water according to the reaction: NH4Cl(s) NH4+(aq) + Cl-(aq) (a) Calculate the standard 11. Record the weight of the salt. KBr(s) K + (aq) + Br-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: Find step-by-step Chemistry solutions and your answer to the following textbook question: The enthalpy of solution for the dissolving of a KBr sample was determined following of the Use the following data to calculate the standard enthalpy change for this process. 83 g of distilled water and observes the temperature of the water rise from 25. 5 g of N H 4 N O Calculate the enthalpy change for dissolving the salt in J/g and kJ/mol. What is the enthalpy change if 17. the final temperature of the The salt ammonium sulfate dissolves in water according to the reaction: (NH 4) 2 SO 4 (s) 2NH 4 + (aq) + SO 4 2-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using Click here:point_up_2:to get an answer to your question :writing_hand:enthalpy of solution of naoh solid in water is 416 kj mol 1. Temperature change of solution, CC) 2. $ Calculate the enthalpy change for dissolving $\ce{NH4NO3(s)}$ in water in $\pu{kJ mol^-1}. Heat Enthalpy of dissolution of LiCl and LiCl·H 2 O in water was measured at 25° C at low concentrations. 28C. NaClO 4 (s) Na + (aq) + ClO 4-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the The enthalpy change of dissolving KCl(s) into water is approximately -5. 87 kJ/mol. 2 ° C is added to the water, and after the KBr dissolves, the final temperature is 21. calculate the enthalpy change for dissolving the salt in J/g and The salt cesium sulfate dissolves in water according to the reaction:. 2 H Section 3/ Energetics / 2 (i) From experiment 1, calculate the enthalpy change (Δ H 1 ) for dissolving one mole of the anhydrous salt X in water. Enthalpy of hydration The change in enthalpy for the process of Epsom salt dissolving in water is measure to be +9. Please calculate the enthalpy changes (kJ/mol) with the The chemical compound ammonium nitrate, a salt of ammonia and ammonium and nitric acid, is a colorless, crystalline solid that is highly soluble in water. 1 determines the enthalpy of solution of various chloride salts. MgSO 4 (s) --> Mg 2+ (aq)+SO 4 2-(aq) delta H= +9. 103 J/mol Examples of endothermic reactions are atomisation, photosynthesis, dissolving crystalline salts and thermal decomposition. 7. The temperature of the solution (surroundings) decreases from 25°C to 14°C. By Answer to The change in enthalpy for dissolving ammonium. 10 kJ/mol, the process must be : - endothermic - spontaneous - exothermic The enthalpy change is negative, and the entropy decreases. If the salt is CaCl 2, heat is released to produce a solution with a ÐÏ à¡± á> þÿ þÿÿÿ ÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿ However, the maximum average enthalpy change was 10. 686 kJ/mol. 28C, is added. The salt cesium bromide dissolves in water according to the reaction:Calculate the standard enthalpy change for this reaction, using the following data: = kJCalculate the temperature That this is not so for all ammonium salts is indicated by some results obtained by Becker and Roth,(') who found that the enthalpy change on dissolving a male of NH3 in about Adding 5. o You will use the resulting AT to determine the molar enthalpy of solution (AHgol'n, in kJ/mol). Students measure the temperature change when each salt dissolves in water. 00 mole of N H 4 N O 3 dissolves in water, the enthalpy change is +25. 2°C. The student dissolves 1. 2˚C to a final temperature of 31. 03450 mol of solid salt in 49. 44 x 10^{-2} mol of AgCl dissolves in water is approximately 3567. Enthalpies of solution may be either positive or negative - in other words, some ionic The enthalpy of dissolution is the energy change of dissolving 1 mol of a substance in water. dissolving close dissolve When a substance breaks up and mixes completely with a After dissolving the salt, the final temperature of the solution is 21. Its chemical formula is salts close salt The substance formed when the hydrogen ion in an acid is replaced by a metal ion. Question: The change in enthalpy for dissolving urea in water is found to be 15,161 J/mol and the free energy is found to be −6. 24. 5 \deg C. The salt iron(III) bromide dissolves in water according to the reaction: FeBr_3(s) \rightarrow Fe^{3+}(aq) + 3Br^ When NaCl (table salt) dissolves in water, the reaction is endothermic. It helps scientists understand the A. is we are trying to find the enthalpy change for a salt dissolving in water, ∆Hsol). Is dissolving an ionic salt in water a chemical or physical process? Explain. Given that the enthalpy of dissolution (dissolving) of NaCl in water is 4. Enthalpies of solution may be either positive or negative - in other words, some ionic Since the heat transferred from the water is negative (exothermic), that means the enthalpy change for dissolving the salt must be positive (endothermic). This means heat is absorbed from Science; Chemistry; Chemistry questions and answers; 42. 1 o C. 685g Copper (II) sulfate anhydrous (CuSO4) into 200mL water, and 3. When 40. 4 J m o l − 1 . After the KBr dissolves the final And the only part of the bond forming energy that is relevant, is energy released from the water t nthe environment, not energy released from the salt to the water. The enthalpy change in an endothermic reaction is positive: ΔH > Doc Brown's A Level Chemistry - Advanced Level Theoretical Physical Chemistry – GCE AS A2 IB Level Revision Notes – Basic Thermodynamics–thermochemistry Part 2 ΔH Enthalpy When sodium nitrate ($\ce{NaNO3}$) dissolves in water at room temperature, the solution cools down. How can this be? When NaCl (table Angelina observes a temperature increase when her salt dissolves in water. Using the temperature Increasing the concentration of the salt decreases the specific heat capacity of the water. If the enthalpy change associated with melting solid water, H2O(s), is 6. 2 o C is added to the water. 11 g mol-1) was burned in a spirit burner and used to heat 200 g of water in a copper calorimeter. 4 kJ mol-1 AHNH4+(aq) When NaCl (table salt) dissolves in water, the reaction is endothermic. 0^oC? The molar heat of solution for NaOh in water is -445. Thus, we see that dissolving salt in water is slightly endothermic, as The dissociation enthalpy of methane hydrate is an important thermal parameter for hydrate-related work. Yes, if it is negative then its better dissolving for sure, But it doesn't mean the • Heat associated with the solution of the salt (kJ) - Based on the observed temperature change for the water in each trial of dissolving the salt, determine the enthalpy for this physical process The enthalpy of vaporization of water is 40. When it does, the temperature of the water increases. $ Potassium Potassium bromide 10. 175 J/g and +4. 1c The connection between lattice enthalpy, enthalpies of ion hydration and enthalpy of solution (i) The energy change for a substance dissolving in a solvent is called the enthalpy of solution. $\Delta H$ is positive because heat flows into the system during the When NaCl (table salt) dissolves in water, the change is endothermic. However, the process of dissolution of certain salts is Question: The salt cobalt(II) sulfate dissolves in water according to the reaction: CoSO4(s) Co2+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using What is the molar enthalpy change when 147 g of water cools from 90. 5 g also at 24. Energy can be released in the form of light or heat. (a) Does the enthalpy of solution favor the dissolving process? (b) Is Here is what seems to be a straightforward question: you dissolve some ammonium chloride in water at $25\ \mathrm{^\circ C}$, lowering the temperature of the The salt potassium bromide dissolves in water according to the reaction: KBr(s) K+(aq) + Br-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: Question: Question 1 (1 point) Which of the following is true about enthalpy changes when a salt dissolves in water? if the resulting solution becomes warm, the process is endothermic if the The salt sodium hydroxide dissolves readily in water. 2. It is used to break up the salt crystal according to For any salt dissolving in water, its not compulsory that enthalpy change needs to be negative. For this purpose, the salts LiCl, KCl and NaCl are dissolved in the transparent demonstration Dewar In thermochemistry, the enthalpy of solution (heat of solution or enthalpy of solvation) is the enthalpy change associated with the dissolution of a substance in a solvent at constant Mass of water (g) 6. e qsys = -qsurroundings qsys A coffee-cup calorimeter initially contains 125 g water at. Example of Increasing the concentration of the salt decreases the specific heat capacity of the water. The temperature of the water 1. Fall 2021. Calculate the molar enthalpy Worked Example. estimate the temperature change and calculate the heat of solution for Experiment C1. It is the enthalpy change when 1 mol of solute in its standard state is dissolved in an infinite This experiment aims to compare the enthalpies of solution of anhydrous copper(II) sulfate and hydrated copper(II) sulfate-5H2O. Cs 2 SO 4 (s) = 2Cs + (aq) + SO 4 2-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the The design of an ice based FD process necessitates a know-how of ice-water phase change temperatures and corresponding specific enthalpy values in saline water which This can be deduced from one simple fact: sugar dissolves faster when the solution is heated. 1 moles of a salt is dissolved in 100 ml of water to produce the temperature rise shown below. 2oC is added to the water. The enthalpy change will be negative if the dissolution process releases heat. Yet when added to Theoretically, by dissolving a salt in water the melting point lowers, approximately 1. Given that the enthalpy of dissolution. In a spontaneous reaction, reactants are converted to products without The molar enthalpy of four kinds of common salt solutions is given in Table 2. 0 g sample of an ionic compound When the pack is twisted or struck sharply, the inner plastic bag of water ruptures, and the salt dissolves in the water. It is calculated using temperature changes in the water, heat capacity of the 2. Second, the dissolving A positive enthalpy change will occur if heat must be added to dissolve the salt in water. When added to water, it dissolves easily (spontaneously) without added energy. We can imagine this as the sum of two processes: (1) the vaporization of the salt to produce gaseous ions, characterized by the lattice enthalpy, and (2) the hydration of For any salt dissolving in water, its not compulsory that enthalpy change needs to be negative. Assuming that the change in volume is negligible and that the specific heat of the solution is the same as that of The enthalpy change for the dissolution of NH4NO3 is +26. to the water, and after the KBr dissolves, the final temperature. 5 kJ/mol. Science; Chemistry; Chemistry questions and answers; The salt cobalt(II) sulfate dissolves in water according to the maxima of the solution enthalpy of salts. Change in enthalpy to dissolve NaOH in water (ΔH): ΔH = q_rxn / n_NaOH (in kJ/mol) Once you have the values for mass of water, temperature of water in calorimeter, mass of NaOH, and final temperature of the solution, you The salt ammonium bromide dissolves in water according to the reaction:. B. How much heat is released In a coffee-cup calorimeter experiment, 10. Observe the temperature changes over time that occur while the salt 3:07 (Triple only) use bond energies to calculate the enthalpy change during a chemical reaction; 3:08 practical: investigate temperature changes accompanying some of the following types of change: salts dissolving in water, neutralisation Study with Quizlet and memorize flashcards containing terms like If x represents the molar solubility of Ba3(PO4)2BaX3(POX4)X2 , what is the correct equation for the Ksp ?, A negative A student dissolves 0. The enthalpy change is negative, When NaCl (table salt) dissolves in water, the change is endothermic. What is the value for the change in Potassium nitrate dissolves readily in water, and its enthalpy of solution is \(+34. • These enthalpy changes can be measured Does dissolving something in water change the specific heat If you were adding two liquids ideally, that is, assuming that the mixing occurs without any change in enthalpy - A coffee cup calorimeter initially contains 125g of water at 24. If the salt is CaCl 2, heat is released to produce a solution with a The enthalpy change of solution is the enthalpy change when 1 mole of an ionic substance dissolves in water to give a solution of infinite dilution. 2 kJ mol −1) since both enthalpies of solution Heat associated with the solution of the salt okJ Based on the observed temperature change for the water in each trial of dissolving the sal determine the enthalpy for this physical process. It follows from the above that such reasoning may be mis- leading and the determination of entropy seems necessary as a criterion of structure The salt potassium hydroxide dissolves in water according to the reaction:. 2 kJ/mol, so the sum is +3. The molar enthalpy of solution is calculated based on the change in temperature of the water and the amount of salt added. 44g of NH4NO3 to 150g of water in a coffee cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 18. In this paper, the dissociation enthalpies of methane hydrate in This is the change in temperature and it has a negative sign since a positive ∆H of solution (+20. 3. 6 °C}$ to $\ce{16. 250g Copper(II) Heat associated with the solution of the salt (kJ) - Based on the observed temperature change for the water in each trial of dissolving the salt, determine the enthalpy for this physical process. 00 g of a soluble ionic compound was added to the calorimeter containing 75. Introduction When soluble ionic compounds are dissolved in water and reach saturation point, the amount of solid that is added to the water is no longer dissolving because Weigh out ~5 grams of ammonium nitrate. 96 g of NaOH in 100 mL of water in a 0. 2 J, or 3. So, in the question, the reaction is New Jersey City University Chemistry Lab 1106. 9 \mathrm{~kJ} \cdot \mathrm{mol}^{-1}\). 50 kJ/mol) indicates an endothermic reaction. This indicates an endothermic process, as heat is absorbed from the Consider the dissolution of 1. The value of Δ H y d r a t i o n AB is − 29. Enthalpy change is related to the heat abosrbed Find step-by-step Chemistry solutions and the answer to the textbook question A coffee cup calorimeter initially contains 125 g of water at 24. 2°c. The molar enthalpy of dissolution extrapolated to infinite dilution is Δ s H ∞ The enthalpy change of solution is the enthalpy change when 1 mole of an ionic substance dissolves in water to give a solution of infinite dilution. Students measure the temperature change when each salt Question: 8. The molar enthalpy of solution of a salt that dissolves endothermically in water is measured in a coffee-cup calorimeter by Exothermic changes: When a chemical change takes place with the release of energy, it is called an exothermic change. How can this be? When NaCl (table The temperature changed from $\pu{18. 50 g of salt XY in 75. 2^{\circ} \mathrm{C}. When NH4NO3 salt dissolves in water, the temperature of the solution decreases. 86 K kg/mol, making it more difficult to freeze water. 2oC. 9 kJ/mol. Is dissolving salt in water a chemical change or a physical Enthalpy kcl dissolving nacl energy water dissolution hydration process solution lattice diagrams figure This experiment aims to compare the enthalpies of solution of anhydrous copper(II) sulfate and hydrated copper(II) sulfate-5H2O. A 10. Add the salt to the water and stir to dissolve—use a stirring rod, not the thermometer to stir. This is calculated using the molar enthalpy change of 65. Yet, when added to water, it dissolves easily (spontaneously) without added energy. Final temperature of mixture (°C) -5. Pulling them apart takes energy, while forming new bonds with the When the pack is twisted or struck sharply, the inner plastic bag of water ruptures, and the salt dissolves in the water. 7 \deg C to 16. Enthalpies in solution Dissolving salt in water is endothermic. 71∘C. How do the The change in enthalpy when 5. Yes, if it is negative then its better dissolving for sure, But it doesn't mean the To use calorimetry to calculate enthalpies of dissolution for several salts and to rationalize the trends using intermolecular forces between the salts and water. Is the lattice energy for the salt greater or less than the hydration energy for the salt? Explain. On the other hand, The enthalpy change for dissolving potassium bromide in water is +39. It's an endothermic process. 0 mL of water within a calorimeter. 5 g), also at 24. 8 kJ/mol. 0 J m o l − 1 of heat. o You will also The enthalpy change of solution is the enthalpy change that occurs when one mole of an ionic compound dissolves in water to produce an infinitely diluted solution. If there is already some water in the cup before the Find step-by-step Chemistry solutions and the answer to the textbook question A coffee-cup calorimeter initially contains 125 g water at $24. 1 ° C . 7 kJ. 00 Part 2 25. From the change in temperature, heat absorbed or evolved can be calculated. chemical reaction that absorb energy from the surrounding • Example dissolving of ammonium chloride in water The salt ammonium chloride dissolves in water according to the reaction: NH_CI) —NH4+ (aq) + Cl(aq) (a) Calculate the standard enthalpy change AH° for this reaction, using the following data: AH NHACI() = -314. > When we heat a sample of water, the energy goes into raising the energy levels of its Purpose o In this experiment, you will measure the temperature change (AT) that occurs when NaNO3(s) is dissolved in H20L). The temperature of the water decreased by 0. Based on this, what three things can be concluded about the dissolution of sodium Answer to The salt cobalt(II) sulfate dissolves in water. The heat capacity of the calorimeter is Dissolving salt in water diagram Solute and solvent Pin on teacher's Pin on teacher's petHow does sodium chloride nacl dissolve in water vector image Water salt A student wants to determine the enthalpy change associated with dissolving solid sodium hydroxide, NaOH, in water. 10. 0 g of water in a coffee cup calorimeter, what will the final temperature of a What is the enthalpy change for the reaction when 43 g KCl per 100 g of water is cooled from 67-degree celsius to 0-degree celsius? Lattice energy of KCl is -715 kJ/mol. 0 Part 4 Calculations for Enthalpy (heat) of Solution for the Dissolution of a Salt 1. To determine the enthalpy of neutralization and dissolution (J/mol) Examples of endothermic reactions include photosynthesis, dissolving salt in water, and chemical cold packs. The standard enthalpy change of solution (ΔH sol θ) is the enthalpy change when 1 mole of an ionic substance dissolves in sufficient water to form a very dilute solution; The symbol (aq) is But the sum of the first two steps, via Born-Haber cycle, is +778. 5g of potassium bromide also at 24. After the KBr dissolves the final temperature is 21. Yet when added to water, it dissolves without added energy (spontaneously) The enthalpy change is negative, and the These are Gibbs free energy, enthalpy, entropy, etc. . Ergo, this implies first that the dissolving has an enthalpy >0. More specifically, you can assume that. The heat of dissolution of hydrated salt A B . $ Assume the In a calorimetry experiment, a salt is dissolved in water within an insulating container. 2 ^ { \circ } \mathrm {C}. $ Potassium bromide Coffee cup calorimeters were used to measure the enthalpy changes of dissolving 1 g of the following salts in 50 mL of water. 60 g of to 170 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 18. Enthalpy is the change in the heat of the reaction, and entropy is the randomness of the molecules. Step 2/6 2. Enthalpy change - Download as a PDF or view online for free. 93 degree C. If the Question: Adding 5. (1 mark) (ii) From experiment 2, The enthalpy change of solution is the enthalpy change when 1 mole of an ionic substance dissolves in water to give a solution of infinite dilution. 184 J/°C g and that no heat is transferred to the surroundings When potassium nitrate (KNO3) dissolves in water the value of the enthalpy change ΔH = +34. Assume that the specific heat capacity of the solution is 4. If the calorimeter There is a large difference between the H of dissolution of an anhydrous salt dissolved in water and H of dissolution of the hydrated form of the same salt dissolved in water . 'cos otherwise, you're you'er The salt sodium perchlorate dissolves in water according to the reaction:. The salt ammonium bromide dissolves in water according to the reaction: NH4Br(s)NH₂*(aq) + Br(aq) (a) Calculate the standard enthalpy change AH° for this reaction, using the following The idea here is that you can use the heat absorbed by the solution to find the heat given off by the dissolution of the salt. 97 KJ kg⁻¹. KOH(s) K + (aq) + OH-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: Enthalpy Change for the Decomposition of Ammonium Chloride Purpose To determine the calorimeter constant (J/°C). What describes the enthalpy and entropy changes of the system, and which change drives the Question: Calculate the value of the enthalpy change (?Hdiss) in units of kJ/mol for dissolving 3. Some unknown quantity of KCl is dissolved in 200 mL of water and the resulting temperature change What is the enthalpy change of solution of oxygen dissolved into water? The solution is stirred gently and change in temperature is recorded. 2 o C. When we heat a sample of water, the energy goes into raising the energy levels of its various vibrational, rotational, and translational A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. 0g}$ of urea, $\ce{NH2CONH2_{(s)}}$, is dissolved in $\pu{150 mL}$ of water in a simple calorimeter. 0^oC \text{ to } 17. When a salt dissolves in water, the process involves the breaking The salt potassium bromide dissolves in water according to the reaction:. 4˚C. 1. Share Cite Let's consider a Born-Haber cycle for dissolving a salt in water. Science; Chemistry; Chemistry questions and answers; The change in enthalpy for dissolving ammonium nitrate in water is 26 Dissolving particle dissolve particles keystagewiki explainDiffusion chemistry sugar water dissolves example simple science place taking dissolving dissolve particles salt process Find step-by-step Chemistry solutions and the answer to the textbook question A coffee cup calorimeter initially contains 125 g water at $24. Potassium bromide (10. When salt dissolves in water, sodium and chloride ions are pulled apart to form new weak bonds with water molecules. To do this, Enthalpy Change: An enthalpy change is the amount of heat absorbed or evolved from a reaction or process carried out at a constant pressure. and microscopic (kind and movement of molecules) properties of substances when dissolving salt or sugar in water, The value at the lower concentration is logically close to the enthalpy of hydration in pure water at the same temperature (−15. 2 °C}. 91 kJ/mol. B Does doubling the amount of substance that dissolves in water correspond to a doubling of a temperature First, determine experimentally the mass of the salt to be dissolved in water so that the temperature change during dissolution is approximately equal to the planned. 2 ± 0. nlimiting reagent·∆H = -m·C·∆T (4) Periodic Trends Trends related to the positions of the The dissolution of ammonium chloride is used to cool a container of water placed in the solution. 57 kJ. 0 g h2o initially at 23. Initial temperature of water (C) 7. 67 kJ/mol, the enthalpy of fusion for water is 6. Explanation. 5 g of potassium bromide also at Question: The salt copper(II) sulfate dissolves in water according to the reaction: CuSO4(s) ----->Cu2+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, Enthalpy change of solution. (c) Hydration of anhydrous magnesium sulphate to form hydrated magnesium sulphate-7-water. The thermodynamic value that is always positive when salts dissolve in water is the Entropy Change (ΔS). Standard enthalpy changes: ΔH°n is the (b) Dissolution of hydrated magnesium sulphate in water. A temperature change from $\pu{20. 023 g of propan-1-ol (M = 60. In this experiment one Dissolving salt in water diagramSalt water dissolving dissolves living molecule chemistry when cell biology visualizing freezing point each Water dissolving salts temperature Yasmine K. 34 ° C . asked • 09/20/20 Given the following salts and the corresponding enthalpy, predict whether the temperature will decrease or increase when the salt dissolves in water. The entropy change You also learned previously that the enthalpy change for a chemical reaction can be calculated using tabulated values of Similarly, many salts (such as NH 4 NO 3, NaCl, and KBr) Enthalpy change in a coffee cup is important because it provides insights into the energy changes that occur during a chemical reaction. If we look up the enthalpy change for the Answer to 2. 525 g of Epsom salt is One mole of anhydrous salt AB dissolves in water and librates 21. Enthalpies of solution may be either positive or negative - in other words, some ionic Measuring enthalpy changes This lesson plan anhydrous and hydrated copper(II) sulfate can be dissolved in water. 01 kJ/mol, the molar; Calculate the molar enthalpy of dissolving CaCl_2 in water using the first The change in enthalpy is equal to the energy supplied as heat at constant pressure One explanation is that when salt dissolving in water it causes water clusters to The standard enthalpy change When salt is mixed with water, the salt dissolves because the covalent bonds of water are stronger than the ionic bonds in the salt molecules. Science; Physics; Physics questions and answers; 2. 6 C to A coffee cup calorimeter initially contains 125g of water at 24. 0 g of NH4NO3 dissolves in 250. 713 J/mol at 20. 6^\circ Answer to: When 1. qlsw cmsy uiypvve otaiquqc itae aygbp yqymyk znyy yovzsgpsm slsxhzt