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The heat of combustion of gaseous methan...

The heat of combustion of gaseous methane `(CH_(4))` at constant volume is measured in bomb calorimeter at 298K is found to be `-885.4kjmol^(-1)`. Find the value of enthalpy change at the same temperature.

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To find the enthalpy change (ΔH) for the combustion of methane (CH₄) at 298 K, we can use the relationship between internal energy change (ΔU) and enthalpy change (ΔH). The formula we will use is: \[ \Delta H = \Delta U + \Delta N_g RT \] Where: - ΔU is the internal energy change (heat of combustion at constant volume), ...
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The heat of combustion of gaseous methan (CH_(4)) at constant volume is measured in a bomb calorimeter at 298 K and is found to be -885.4 kJ mol^(-1) .Find the value of enthalpy change.

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Knowledge Check

  • Heat of combustion of ethanol at constant pressure and at temperature T K(=298 K) is found to be -qJ "mol"^(-1) . Hence , heat of combustion (in J "mol"^(-1) ) of ehtanol at the same temperature at constant volume will be:

    A
    RT-q
    B
    `-(q+RT)`
    C
    q-RT
    D
    q+RT

  • Heat of combustion of ethanol at constant pressue and at temperature TK(=298K) is found to be -qJmal^(-1) . Hence, heat of combustion (in Jmol^(-1) ) of ethanol at the same temperature at constant volume will be:

    A
    `RT-q`
    B
    `-(q+RT)`
    C
    `q-RT`
    D
    `q+RT`

  • Heat of combustion of ethanol at constant pressure and at temperature TK is found to be -q J" mol"^(-1) . Hence, heat of combustion (in J mol^(-1) ) of ethanol at the same temperature and at constant volume will be :

    A
    `RT-q`
    B
    `-(q+RT)`
    C
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