Thursday
July 31, 2014

Homework Help: chemistry

Posted by Anonymous on Wednesday, July 16, 2008 at 8:25pm.

A calorimeter consists of an interior metal bomb (container) surrounded by 2.22 kg of water all contained within an insulated exterior wall. A sample of propane, C3H8, weighing 6.89g, was burned in the calorimeter with excess oxygen. As a result of the combustion, the interior temperature rose from 23.61*C to 26.88*C. It can be assumed that there is no heat loss to the exterior wall nor to the surroundings. The heat capacity of the metal bomb and contents is 337 cal/*C. The specific heat of water at 25*C is 0.998 cal/g*C. Calculate the following. A) The change in temperature [26.88*C-23.61*C=3.27*C] B)The heat absorbed by the water in calories. [Q=delta T(m)(Csp) (3.27*C)[(2.22kg)(1000g/kg)](0.998cal/g*C)=7.24x10^3 cal] C)The heat absorbed by the metal bomb and contents in calories [(3.27*C)(337 cal/*C)=1.10x10^3 cal] D) The total heat absorbed by the calorimeter in calories [7.24x10^3 cal + 1.10x10^3 cal= 8.34x10^3 cal] E) The moles of propane burned [6.89 g C3H8 x 1mol/ (3*12.01 + 8*1.008)gC3H8 = .156 mol C3H8] F)The heat of combustion of propane in kcal/mol. G)The heat of combustion of propane in kJ/mol

Can you check parts a through e? I'm not sure if I did them correctly. I don't know how to do parts f and g. Thanks for the help!

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