Home
Class 12
CHEMISTRY
In a constant volume calorimeter, 3.5 g ...

In a constant volume calorimeter, `3.5 g` of a gas with molecular weight `28` was burnt in excess oxygen at `298.0 K`. The temperature of the calorimeter was found to increase from `298.0 K to 298.45 K` due to the combustion process. Given that the heat capacity of the calorimeter is `2.5 kJ K^(-1)`, find the numerical value for the enthalpy of combustion of the gas in `kJ mol^(-1)`

Promotional Banner

Similar Questions

Explore conceptually related problems

In a constant volume calorimeter, 3.5g of a gas with molecular mass 28 was burnt in excess oxygen at 298.0 K. the temperature of the calorimeter was found to increase from 298.0K to 298.45K, due to the combustion process. Given, that the heat capacity of the calorimeter is 2.5kJ*K^(-1) , what will be the value of enthalpy of combustion of the gas?

In a constant volume calorimeter 5g of a gas with molecular weight 40 was burnt in excess of oxygen at 298 K.the temperature of the calorimeter was found to increase from 298 K to 298.75 K due to combustion process.Given that the heat capacity of the calorimeter is 2.5 kJ K^(-1),a numerical value for the DeltaU of combustion of the gas in kJ mol^(-1) is