Suppose you burned 0.300 g of in an excess of in a constant-volume calorimeter to give .

C(s) ->O2(g)->CO2(g)

The temperature of the calorimeter, which contained 749 g of water, increased from 26.55 C to 29.00 C. The heat capacity of the bomb is 890. J/K. Calculate per mole of carbon. (The specific heat capacity of liquid water is 4.184 J/g K.)

Suppose you burned 0.300g of C(s) in an excess of O2(g) in a constant-volume calorimeter to give CO2(g). C(s)+O2(g)CO2(g) The temperature of the calorimeter, which contained 749g of water, increased from 26.55C to 29.00C. The heat capacity of the bomb is 890.1/K. Calculate 6 per mole of carbon. (The specific heat capacity of liguid water is 4.184J/gK.) U=k/molC