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The heat of combusion of benzene in a bo...

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 .

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To calculate the heat of combustion of benzene at constant pressure (ΔH) from the heat of combustion at constant volume (ΔU), we can use the following relationship: \[ \Delta H = \Delta U + \Delta n_g \cdot R \cdot T \] Where: - ΔH = heat of combustion at constant pressure ...
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The heat produced by the combustion of 2.0g of benzene in a bomb calorimeter was found to be 123.6 kJ at 25^(@)C . Calculate the enthalpy of combustion of benzene at 25^(@)C .

The combustion of benzene (l) gives CO_(2)(g) and H_(2)O(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)

The heat liberated on complete combustion of 7.8g benzene is 327kJ . This heat has been measured at constant volume and at 27^(@)C . Calculate heat of combustion of benzene at constant pressure at 27^(@)C . (R=8.3 J mol^(-1)K^(-1))

The heat liberated on complete combustion of 7.8g benzene is 327kJ . This heat has been measured at constant volume and at 27^(@)C . Calculate heat of combustion of benzene at constant pressure at 27^(@)C . (R=8.3 J mol^(-1)K^(-1))

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))

When 2 g of benzene are burnt in a bomb calorimeter, the heat produced is 83.6 kJ at 298 K. Calculate the enthalpy of combustion of benzene.

0.16 g of methane was subjected to combustion at 27°C in a bomb calorimeter. The temperature of the calorimeter system (including water) was found to rise by 0.5°C. Calculate the heat of combustion of methane (i) at constant volume and (ii) at constant pressure. The thermal capacity of the calorimeter system is 17.7 kJ K^(-1)(R = 8.314 JK^(-1) mol^(-1)) .

A sample of 0.16 g CH_(4) was subjected to combustion at 27^(@)C in a bomb calorimeter. The temperature of the calorimeter system (including water) was found to rise by 0.5^(@)C . Calculate the heat of combustion of methane at (a) constant volume and (b) constant pressure. The thermal capacity of calorimeter system is 17.7 kJ K^(-1) and R = 8.314 J K^(-1) mol^(-1) .

A sample of 0.16 g CH_(4) was subjected to combustion at 27^(@)C in a bomb calorimeter. The temperature of the calorimeter system (including water) was found to rise by 0.5^(@)C . Calculate the heat of combustion of methane at (a) constant volume and (b) constant pressure. The thermal capacity of calorimeter system is 17.0 kJ K^(-1) and R = 8.314 J K^(-1) mol^(-1) .

0.5 g of benzoic acid was subjected to combustion in a bomb calorimeter at 15^(@)C when the temperature of the calorimeter system (including water) was found to rise by 0.55^(@)C . Calculate the heat of combustion of benzoic acid (i) at constant volume and (ii) at constant pressure. the thermal capacity of the calorimeter including water was found to be 23.85 kJ.

VMC MODULES ENGLISH-THERMOCHEMISTRY-JEE ADVANCED (ARCHIVE)
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  2. The enthalpies for the following reactions (DeltaH^(Theta)) at 25^(@)C...

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  3. (A) The standard heats of formation of at 298 K for CCI(4)(g), H(2)O(g...

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