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1. Determine the enthalpy change for NaOH (s) + HCl (aq) → NaCl (aq) + H2O (l) using Hess's Law.
a. Write the balanced chemical reaction and enthalpy change for Part I (1pt)
b. Write the balanced chemical reaction and enthalpy change for Part II (1pt)
c. Calculate the enthalpy change using Hess's Law. Refer to the lesson for an example of Hess's Law. (2pt)
2. If the accepted enthalpy change value for the dissolving of sodium hydroxide in water is −44.2 kilojoules per mole, determine the percent error of the experimental value that you calculated in Part I. Show your work.
(experimental - actual value) / actual value × 100 %
3. If the accepted heat of reaction for the neutralization of hydrochloric acid with sodium hydroxide is −56.0 kilojoules per mole, determine the percent error of the experimental value that you calculated in Part II. Show your work.
(experimental - actual value) / actual value × 100 %
4. Using the accepted values of the processes you've examined, would your estimation of the enthalpy change for the reaction of solid sodium hydroxide in aqueous hydrochloric acid change from the prediction you made in question one? Explain your answer in complete sentences.
5. Give a detailed explanation, using what you know about bonds and forces of attraction, for the enthalpy
1. Determine the enthalpy change for NaOH (s) + HCl (aq) → NaCl (aq) + H2O (l) using Hess's Law.
a. Write the balanced chemical reaction and enthalpy change for Part I (1pt)
b. Write the balanced chemical reaction and enthalpy change for Part II (1pt)
c. Calculate the enthalpy change using Hess's Law. Refer to the lesson for an example of Hess's Law. (2pt)
2. If the accepted enthalpy change value for the dissolving of sodium hydroxide in water is −44.2 kilojoules per mole, determine the percent error of the experimental value that you calculated in Part I. Show your work.
(experimental - actual value) / actual value × 100 %
3. If the accepted heat of reaction for the neutralization of hydrochloric acid with sodium hydroxide is −56.0 kilojoules per mole, determine the percent error of the experimental value that you calculated in Part II. Show your work.
(experimental - actual value) / actual value × 100 %
4. Using the accepted values of the processes you've examined, would your estimation of the enthalpy change for the reaction of solid sodium hydroxide in aqueous hydrochloric acid change from the prediction you made in question one? Explain your answer in complete sentences.
5. Give a detailed explanation, using what you know about bonds and forces of attraction, for the enthalpy