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Heat of combustion of CH4(g) at constant...

Heat of combustion of `CH_4`(g) at constant volume and at 298 K has been found to be -`885 kJ mol^(-1)`, calculate the enthalpy of its combustion under constant pressure condition (`R = 8.31 J K^(-1) mol^(-1)`).

Text Solution

AI Generated Solution

To calculate the enthalpy of combustion of methane (CH₄) under constant pressure conditions, we can use the relationship between the internal energy change (ΔE) and the enthalpy change (ΔH). The formula we will use is: \[ \Delta H = \Delta E + \Delta N_g \cdot R \cdot T \] Where: - ΔH = Enthalpy change ...
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The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .

The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .

Knowledge Check

  • The combustion of benzene(/) gives CO_2(g) and H_2O(l) Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol^(-1) at 25^@C , heat of combustion (in kJ mol^(-1) ) of benzene at constant pressure will be (R = 8.314 JK^(-1) mol^(-1))

    A
    `4152.6`
    B
    `-452.46`
    C
    `3260`
    D
    `-3267.6`

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