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3. The following acid and base solutions are placed in a calorimeter at constant pressure: 50.0 mL of 0.20 M HCl and 50.0 mL of 0.30 M NaOH. The water in the mixture has a specific heat of 4.184 J/g C. The water is initially at 21.0 C and at the end of the reaction is at 24.7 C. a. Write the balanced chemical equation for the reaction. Include states of matter. b. Calculate the heat q for this reaction using the calorimetry equation. Assume the density of each solution is 1.0 g/mL (d=m/V). C. Calculate the number of moles of HCl used in the reaction. d. Calculate the moles of NaOH used in the reaction. e. Use the relation q +4H = 0 to find the enthalpy change for the reaction f. Find the molar heat of reaction by using AH/n where n is the number of moles of the limiting reactant. Recall that the limiting reactant is the reactant that produces the smaller amount of products in a reaction. Enter

3. The following acid and base solutions are placed in a calorimeter at constant pressure: 50.0 mL of 0.20 M HCl and 50.0 mL of 0.30 M NaOH. The water in the mixture has a specific heat of 4.184 J/g C. The water is initially at 21.0 C and at the end of the reaction is at 24.7 C. a. Write the balanced chemical equation for the reaction. Include states of matter. b. Calculate the heat q for this reaction using the calorimetry equation. Assume the density of each solution is 1.0 g/mL (d=m/V). C. Calculate the number of moles of HCl used in the reaction. d. Calculate the moles of NaOH used in the reaction. e. Use the relation q +4H = 0 to find the enthalpy change for the reaction f. Find the molar heat of reaction by using AH/n where n is the number of moles of the limiting reactant. Recall that the limiting reactant is the reactant that produces the smaller amount of products in a reaction. Enter

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.109QP: A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter...
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1 Normal 1 No Spac. Heading 1 Heading 2 三、 Styles Paragraph 3. The following acid and base solutions are placed in a calorimeter at constant pressure: 50.0 mL of 0.20 M HCl and 50.0 mL of 0.30 M NaOH. The water in the mixture has a specific heat of 4.184 J/g C. The water is initially at 21.0 C and at the end of the reaction is at 24.7 C. a. Write the balanced chemical equation for the reaction. Include states of matter. b. Calculate the heat q for this reaction using the calorimetry equation. Assume the density of each solution is 1.0 g/mL (d3m/V). C. Calculate the number of moles of HCl used in the reaction. d. Calculate the moles of NaOH used in the reaction. e. Use the relation q +4H = 0 to find the enthalpy change for the reaction f. Find the molar heat of reaction by using AH/n where n is the number of moles of the limiting reactant. Recall that the limiting reactant is the reactant that produces the smaller amount of products in a reaction. (Ctrl) - Enter response here
Transcribed Image Text:1 Normal 1 No Spac. Heading 1 Heading 2 三、 Styles Paragraph 3. The following acid and base solutions are placed in a calorimeter at constant pressure: 50.0 mL of 0.20 M HCl and 50.0 mL of 0.30 M NaOH. The water in the mixture has a specific heat of 4.184 J/g C. The water is initially at 21.0 C and at the end of the reaction is at 24.7 C. a. Write the balanced chemical equation for the reaction. Include states of matter. b. Calculate the heat q for this reaction using the calorimetry equation. Assume the density of each solution is 1.0 g/mL (d3m/V). C. Calculate the number of moles of HCl used in the reaction. d. Calculate the moles of NaOH used in the reaction. e. Use the relation q +4H = 0 to find the enthalpy change for the reaction f. Find the molar heat of reaction by using AH/n where n is the number of moles of the limiting reactant. Recall that the limiting reactant is the reactant that produces the smaller amount of products in a reaction. (Ctrl) - Enter response here
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