The bomb calorimeter in Exercise 87 is filled with 987 g of water. The initial temperature of the calorimeter contents is 23.32oC. A 1.056-g sample of benzoic acid (ΔEcomb = 226.42 kJ/ g) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?
Answer to relevant QuestionsIf a student performs an endothermic reaction in a calorimeter, how does the calculated value of ΔH differ from the actual value if the heat exchanged with the calorimeter is not taken into account? Using the following data, calculate the standard heat of formation of ICl(g) in kJ/ mol: Cl2(g) → 2Cl(g) ΔHo = 242.3 kJ I2(g) → 2I(g) ΔHo = 151.0 kJ ICl(g) → I(g) + Cl(g) ΔHo = 211.3 kJ I2(s) → I2(g) ΔH8 = 62.8 ...The heat of vaporization of water at the normal boiling point, 373.2 K, is 40.66 kJ/mol. The specific heat capacity of liquid water is 4.184 JK-1g-1 and of gaseous water is 2.02 J K-1g-1. Assume that these values are ... A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapor. Given the following data, determine ΔHof for the hydrocarbon: ΔHrxn = –2044.5 kJ/ mol ΔHof (CO2) = –393.5 kJ/ mol ΔHof ...A cylinder with an initial volume of 10.0 L is fitted with a frictionless piston and is filled with 1.00 mole of an ideal gas at 25oC. Assume that the surroundings are large enough so that if heat is withdrawn from or added ...
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