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Let's use calorimetry to measure heats of reaction but this time let's have a limiting reactant. Review #3 in T8VE if you want. Suppose you mix 25.0 mL of 0.12M cesium hydroxide with 25.0 mL of 0.30M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 31.3°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q as positive it you thought the reaction was endothermic and negative if you thought it was exothermic. The Q is The heat of the reaction is generally reported as heat per mole. The moles of acid are Look at your moles and pick the limiting reactant. Therefore the heat of the reaction (in kJ/mole) is Joules. and the moles of base are Subm

Let's use calorimetry to measure heats of reaction but this time let's have a limiting reactant. Review #3 in T8VE if you want. Suppose you mix 25.0 mL of 0.12M cesium hydroxide with 25.0 mL of 0.30M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 31.3°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q as positive it you thought the reaction was endothermic and negative if you thought it was exothermic. The Q is The heat of the reaction is generally reported as heat per mole. The moles of acid are Look at your moles and pick the limiting reactant. Therefore the heat of the reaction (in kJ/mole) is Joules. and the moles of base are Subm

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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8:34 PM Sun Oct 23 T27HW Question 9 Unanswered Let's use calorimetry to measure heats of reaction but this time let's have a limiting reactant. Review #3 in T8VE if you want. Suppose you mix 25.0 mL of 0.12M cesium hydroxide with 25.0 mL of 0.30M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 31.3°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q as positive if you thought the reaction was endothermic and negative if you thought it was exothermic. The Q is The heat of the reaction is generally reported as heat per mole. The moles of acid are Look at your moles and pick the limiting reactant. Therefore the heat of the reaction (in kJ/mole) is Joules. 50% and the moles of base are Submit
Transcribed Image Text:8:34 PM Sun Oct 23 T27HW Question 9 Unanswered Let's use calorimetry to measure heats of reaction but this time let's have a limiting reactant. Review #3 in T8VE if you want. Suppose you mix 25.0 mL of 0.12M cesium hydroxide with 25.0 mL of 0.30M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 31.3°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q as positive if you thought the reaction was endothermic and negative if you thought it was exothermic. The Q is The heat of the reaction is generally reported as heat per mole. The moles of acid are Look at your moles and pick the limiting reactant. Therefore the heat of the reaction (in kJ/mole) is Joules. 50% and the moles of base are Submit
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