Home
Class 12
CHEMISTRY
When 1.0g of a compound (molecular weigh...

When 1.0g of a compound (molecular weight=28) is burnt in a bomb calorimeter, the temperature of the calorimeter rises from `25^(@)C` to `25.45^(@)C`. Calculate the heat that evolves when 1 mol of this compound is completely burnt `(C_(cal)=2.5kJ*K^(-1))`.

Text Solution

Verified by Experts

`DeltaT=[(372+25.45)-(273+25)]=0.45K`
Therefore, heat evolved due to combustion of 1 g of the compound`=C_(cal)xxDeltaT=2.5kJ*K^(-1)xx0.45K=1.125kJ`.
`therefore` Heat produced due to combustion of 1 mol or 28g of that compound`=1.125xx28=31.5kJ`.
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS

    CHHAYA PUBLICATION|Exercise WARM UP EXERCISE|119 Videos

  • CHEMICAL THERMODYNAMICS

    CHHAYA PUBLICATION|Exercise QUESTION ANSWER ZONE FOR BOARD EXAMINATION (VERY SHORT ANSWER TYPE)|26 Videos

  • CHEMICAL KINETICS

    CHHAYA PUBLICATION|Exercise EXERCISE (NUMERICAL PROBLEMS)|37 Videos

  • CHEMISTRY IN EVERYDAY LIFE

    CHHAYA PUBLICATION|Exercise PRACTICE SET 15|15 Videos

Similar Questions

Explore conceptually related problems

When 1 g of graphite is completely burnt in a bomb calorimeter, the temperature of the bomb and water rises from 25^(@)C to 30.5^(@)C . If the heat capacity of the calorimeter is 5.96kJ*""^(@)C^(-1) , then the heat of combustion per mole of graphite at constant volume is-

When a gas (molar mass =28g*mol^(-1) ) of mass 3.5 is burnt completely in presence of excess oxygen in a bomb calorimeter, the temperature of the calorimeter increases from 298 K to 298.45 K. the heat of combustion at constant volume for the gas (Given: heat capacity of the calorimeter =2.5kJ*K^(-1) ) is-

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?

At 25^(@)C the heat of combustion at constant volume of 1 mol of a compound is 5150 kJ. The temperature of a bomb calorimeter rises from 25^(@)C to 30.5^(@)C when a certain amount of the compound is burnt in it. If the heat capacity of the calorimeter is 9.76 kJ*K^(-1) then how much of the compound was taken for combustion. [Molar mass of the substance=128]

2 g of an organic compound is burnt completely in a bomb calorimeter at 289 K. The final temperature of calorimeter was found to be 298.5 K. Calorimeter constant is 400JK^-1 and molar mass of the compound is 50 g. What is the enthalpy of combustion per mol of the compound in kJ unit?

Calculate the number of kJ necessary to raise the temperature of 60g of aluminium from 35^(@)C to 55^(@)C . Molar heat capacity of Al is 24J*mol^(-1)*K^(-1) .

How many calories are required to increase the temperature of 40g of Ar from 40^(@)C to 100^(@)C at a constant volume (R=2cal*mol^(-1)*K^(-1)) -

The temperature of 1 mol of an ideal monoatomic gas at constant pressure of 1 atm changes from 25^(@)C and 50^(@)C . Calculate Delta U and Delta H in this process, (C_(V)=(3)/(2)R) .

Calculate the number of kJ of heat necessary to raise the temperature of 60.0 g of aluminium from 35^@C to 55^@C . Molar heat capacity of Al is 24 J mol^-1 K^-1 . Molar mass of Al =27g mol^-1 .