Home
Class 11
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)`

Text Solution

AI Generated Solution

To find the enthalpy of combustion of the gas in kJ/mol, we can follow these steps: ### Step 1: Calculate the number of moles of the gas Given: - Mass of the gas = 3.5 g - Molecular weight of the gas = 28 g/mol The number of moles (n) can be calculated using the formula: ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Archives (Fill In The Blanks)|5 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Archives (True/False)|2 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Archives (Assertion-Reasoning)|3 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

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

Knowledge Check

  • In a constant volume calorimeter, 3.5g 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 K to 298 K due to the combustion process. Given that the combustion process. Given that the heat capacituy of the calorimeter is 2.5 J K^(-1) , the value for the enthalpy of combustion of the gas id

    A
    `90 kJ mol^(-1)`
    B
    `9 kJ mol^(-1)`
    C
    `18 kJ mol^(-1)`
    D
    `6 kJ mol^(-1)`

  • 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

    A
    15
    B
    12
    C
    90
    D
    8

    • Similar Questions

    Explore conceptually related problems

    In a constant volume calorimeter, 3.5 g of a gas with moleular 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 KJK^(-1) , the numerical value for the enthalphy of combustion of the gas in KJ mol^(-1) is .

    In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burtn in excess oxygen at 298.0 K. The temperaure of the calorimeter was found to increase from 298.0 Kto298.45 K due to the combustion process.Given that the heat energy capacity of the calorimeter is 2.5 kJ K^(-1) , the numerical value for the enthalpy of combustion of the gas in kJ mol^(-1) is

    In a constant volume calorimeter, 3.5g 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 298.0K to 298.45 K due to the combustion of the gas in kJ mol^(-1) is

    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 process. Given that the heat capacity of the calorimeter is 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) , the numerical value for the enthalpy of combustion of the gas in kJ "mol"^(-1) is

    A 1.25g sample of octane (C_(8)H_(18)) is burnt in excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rises from 294.05 to 300.78 K. If heat capacity of the calorimeter is 8.93 kJ K^(-1) . Find the heat transferred to calorimeter.

    A 1.250 g sample of octane (C_(8)H_(18)) is burnedin excess of oxygen in a bomb calorimeter. The temperatre of the calorimeter rises from 294.05 K to 300.78K. If heat capacity of the calorimeter is 8.93kJ // K, find the heat transferred to the calorimeter. Also calculate the enthalpy combustion of the sample of octane.

    Home
    Profile