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When 0 cdot 5 g of sulphur is burnt to f...

When `0 cdot 5` g of sulphur is burnt to from `SO_2(g), 4 cdot k` of heat is liberated. The enthalpy of formation of `SO_2(g)` is:

A

`-147 cdot 2` k J

B

`+ 147 cdot 2` k J

C

`+294 cdot 4` k J

D

`-294 cdot 4` k J

Text Solution

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The correct Answer is:
D
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From the data given below at 298 K for the reaction : CH_(4)(g) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l) Calculate the enthalpy of formation of CH_(4)(g) at 298 K. Enthalpy of reaction is = -893.5 kJ Enthalpy of formation of CO_(2)(g) = 393. kJ mol^(-1) Enthalpy of formation of H_(2)O(l) = 286.0 kJ mol^(-1) .

The number of moles in 0.64 g of SO_2 is :

Knowledge Check

  • When 0.5 g of sulphur is burnt to SO_(2):4.6 kJ of heat is liberated. What is the enthalpy of formation of sulphur dioxide ?

    A
    `-147.2 kJ`
    B
    `+147.2 kJ`
    C
    `+294.4 kJ`
    D
    `-294.4 kJ`

  • In the combustion of 4g of CH_4, 2cdot 5 kcal of heat is liberated. The heat of combustion of CH_4 is

    A
    `0 cdot 1 kcal mol^(-1)`
    B
    `10 kcal mol^(-1)`
    C
    `1 cdot 0 kcal mol^(-1)`
    D
    `100 kcal mol^(-1)`

  • In order to decompose 9 g of water, 142 cdot 5 k J of heat is required. Hence enthalpy of formation of water is:

    A
    `- 142 cdot 5` k J
    B
    `+142 cdot 5` k J
    C
    - 285 k J
    D
    + 285 k J

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