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Calculate the ethalpy of combustion of e...

Calculate the ethalpy of combustion of ethylene (g) to form `CO_(2)` (gas) and `H_(2)O` (gas) at 298 K and 1 atmospheric pressure. The enthalpies of formation of `CO_(2),H_(2)O` and `C_(2)H_(4)` are `-393.7, -241.8+52.3` kJ per mole respectively.

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To calculate the enthalpy of combustion of ethylene (C₂H₄) to form carbon dioxide (CO₂) and water (H₂O) at 298 K and 1 atmospheric pressure, we can follow these steps: ### Step 1: Write the balanced chemical equation for the combustion of ethylene. The combustion of ethylene can be represented by the following reaction: \[ \text{C}_2\text{H}_4(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \] ...
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Calculate the enthalypy of combustion of ethylene (gas) to form CO_(2) (gas ) and H_(2) O (gas) at 298 K and 1 atmospheric pressure. The enthalpies of formation of CO_(2), H_(2)O and C_(2)H_(4) are - 393.7, -241.8 ,+52.3kJ per mole respectively.

Calculate the heat of combustion of 1 mole of C_(2)H_(4)(g) to form CO_(2)(g) and H_(2)O(g) at 398K and 1 atmosphere, given that the heats of formation of CO_(2)(g),H_(2)O(g) and C_(2)H_(4)(g) are -94.1,-57.8 and +12.5kcal" "mol^(-1) respectively.

Knowledge Check

  • The heats of combustion for C, H_(2) and CH_(4) are -349, -241.8 and -906.7 kJ respectively. The heat of formation of CH_(4) is

    A
    174.1 kJ
    B
    274.1 kJ
    C
    374.1 kJ
    D
    74.1 kJ

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    Calculate the standard enthalpy of formation of ethylene, C_(2)H_(4)(g) from the following thermochemical equation : C_(2)H_(4)(g) + 3O_(2)(g) to 2CO_(2)(g) + 2H_(2)O(g) Delta_(r)H^(@) = -1323 kJ Given the standard enthalpy of formation of CO_(2)(g) and H_(2)O(g) are - 393.5 and -249 kJ mol^(-1) respectively.

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