Home
Class 11
CHEMISTRY
1g of graphite is burnt in a bomb calori...

1g of graphite is burnt in a bomb calorimeter in excess of oxygen at 298 K and 1 atmospheric pressure according to the equation
C (graphite)`+O_(2)(g)rarrCO_(2)(g)`
During the reaction, temperature rises from 298 K to 299 K. If the heat capacity of the bomb calorimeter is 20.7kJ/K, what is the enthalpy change for the above reaction at 298 K and 1 atm?

Text Solution

Verified by Experts

Rise in temperature in calorimeter = `299-298K=1K`
Heat capacity of the calorimeter = `20.7KJ K^(-1)`
`therefore` Heat absorbed by the calorimeter =
`C_(V)DeltaT=(20.7KJK^(-1))(1K)=20.7K`
This is the heat evolved in the combustion of 1g of graphite
`therefore` Heat evolved in the combustionof 1 mole of graphite.
i.e 12g of graphite = `20.7xx12KJ=248.4KJ`
As this is the heat evolved and the vessel is closed, therefore, enthalpy change of the reaction `(DeltaU)` `=-248.4KJmol^(-1)`
Promotional Banner

Similar Questions

Explore conceptually related problems

0.562g of graphite kept in a bomb calorimeter in excess of oxygen at 298K and 1 atmospheric pressure was burnt according to the equation, C_(Graph ite)+O_(2(g))rarr CO_(2(g)) durgin the reaction, temperature rises from 298K o 298.89K . If the heat capacity of the calorimeter and its contents is 20.7 kJ//K , what is the enthalpy change for the above reaction at 298K and 1 atm ?

The standard enthalpy of diamond is zero at 298K and 1 atm pressure.

Four grams of graphite is burnt in a bomb calorimeter of heat capacity of 30 kJ K^(-1) 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 "mol6(-1) )?

Four grams of graphite is burnt in a bomb calorimeter of heat capacity 30kJK^(-1) is 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"^(-1) )?

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)