Don't use AI Before you enter the lab, it is important to know hiw tocalibrate your calorimeter. Determine the calorimeterconstsnt if dodecane was used as a fuel using theinfirmation provided.

The calorimeter constant (heat capacity of the calorimeter), can be calculated using the…

Answered: Before you enter the lab, it is…

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 7RQ: Explain how calorimetry works to calculate H or E for a reaction. Does the temperature of the...

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Similar questions

Explain why H is obtained directly from coffee-cup calorimeters, whereas E is obtained directly from bomb calorimeters.
Explain why the specific heat of the contents of the calorimeter must be known in a calorimetry experiment.
An exothermic reaction is carried out in a coffee-cup calorimeter. Which of the following statements is/are NOT true for the process? (a) The temperature of the water increases. (b) Heat is absorbed by the water. (c) The enthalpy of the products is higher than the enthalpy of the reactants. (d) qH2o=qrxn (e) qrxn0 (f) qrxn+qH2o=0
9.65 When 0.0157 g of a compound with a heat of combustion of —37.6 kJ/mol is burned in a calorimeter, 18.5 j of heat is released. What is the molar mass of the compound?
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
How much heat is produced by combustion of 125 g of methanol under standard state conditions?
The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the calorimeter contents is 23.32C. A 1.056-g sample of benzoic acid (Ecomb = 26.42 kJ/g) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?
A compound is 82.7% carbon and 17.3% hydrogen, and has a molar mass of approximately 60 g/mol. When 1.000 g of this compound burns in excess oxygen, the enthalpy change is 49.53 kJ. (a) What is the empirical formula of this compound? (b) What is the molecular formula of this compound? (c) What is the standard enthalpy of formation of this compound? (d) Two compounds that have this molecular formula appear in Appendix G. Which one was used in this exercise?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.
Explain how calorimetry works to calculate H or E for a reaction. Does the temperature of the calorimeter increase or decrease for an endothermic reaction? For an exothermic reaction? Explain.
Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB. A2(aq)+B2(aq)2AB(aq);H=+271kJ/mol If solutions A2(aq) and B2(aq), starting at the same temperature, are mixed in a coffee-cup calorimeter, the reaction that occurs is a exothermic, and the temperature of the resulting solution rises. b endothermic, and the temperature of the resulting solution rises. c endothermic, and the temperature of the resulting solution falls. d exothermic, and the temperature of the resulting solution falls. e exothermic or endothermic, depending on the original and final temperatures.
Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.

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Before you enter the lab, it is important to know hiw to calibrate your calorimeter. Determine the calorimeter constsnt if dodecane was used as a fuel using the infirmation provided.