Four grams of graphite is burnt in a bomb calorimeter of heat capacity 30KJ/mol in excess of oxygen at 1 atmospheric pressure. The temperature rises from 300 to 304 K.what is the enthalpy of combustion of graphite (in KJ /mol)

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Solution

$E n t h a l p y o f c o m b u s t i o n = q \times m \times ∆ T = 30 \times 4 \times (304 - 300) = 30 \times 4 \times 4 = 480 k J$

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Q. 1 g of graphite is burnt in a bomb calorimeter in excess of oxygen at 298 K and 1 atmospheric pressure according to the equation

C (g r a p h i t e) + O_{2} (g) \to {C O}_{2} (g)

During the reaction, temperature rises from 298 K to 299 K. If the heat capacity of the bomb calorimeter is 20.7 kJ/K, what is the enthalpy change for the above reaction at 298 K and 1 atm?

In a constant volume calorimeter, $3.5 g$ of a gas with molecular weight 28 g/mol was burnt in excess of oxygen at $298 K$ . The temperature of the calorimeter was found to Increase from $298 K$ to $298.45 K$ due to the combustion process. Given that the heat capacity of the calorimeter is $2.5 k J / K$ . The Numerical value for the enthalpy of combustion of the gas in kJ/mol is