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Given C (graphite) + O(2) (g) to CO(2) (...

Given C (graphite) `+ O_(2) (g) to CO_(2) (g) Delta ""_(r) H^(0) = -393.5 k J * mol^(-1)`
`H_(2) (g) + (1)/(2) O_(2) (g) to H_(2) O (l) , Delta ""_(r) H^(0) = -285.8 kJ * mol^(-1)`
`CO_(2) (g) + 2 H_(2) O(l) to CH_(4) + 2 O_(2) (g) , Delta ""_(r)H^(0) = + 890 . 3 kJ * mol^(-1)`
Based on the above thermochemical equations , the value of `Delta ""_(r) H^(0)` at 298 K for the reation C(graphite) + `2 H_(2) (g) to CH_(4) (g)` will be -

A

`-74.8 kJ * mol^(-1)`

B

`-144.0 kJ * mol^(-1)`

C

`+ 74. 8 kJ * mol^(-1)`

D

`+ 144.0 kJ * mol^(-1)`

Text Solution

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Knowledge Check

  • Given, C(graphite)+ O_(2)(g)toCO_(2)(g),Delta_(r)H^(0)=-393.5kJ*mol^(-1) H_(2)(g)+(1)/(2)(g)toH_(2)O(l),Delta_(r)H^(0)=-285.8kJ*mol^(-1) CO_(2)(g)+2H_(2)O(l)toCH_(4)(g)+2O_(2)(g),Delta_(r)DeltaH^(0)=+890.3kJ*mol^(-1) Based on the above thermochemical equations, the value of Delta_(r)H^(0) at 298K for the reaction, C(graphite) +2H_(2)(g)toCH_(4)(g) , will be-

    A
    `-74.8kJ*mol^(-1)`
    B
    `-144.0kJ*mol^(-1)`
    C
    `+74.8kJ*mol^(-1)`
    D
    `+144.0kJ*mol^(-1)`

  • Given (at 25^(@)C ): Ca(s)+(1)/(2)O_(2)(g)toCaO(s),DeltaH^(0)=-635.2kJ*mol^(-1) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),DeltaH^(0)=-285.8kJ*mol^(-1) CaO(s)+H_(2)O(l)toCa(OH)_(2)(s) , DeltaH^(0)=-65.6kJ*mol^(-1) The heat of formation (in kJ*mol^(-1) ) for Ca(OH)_(2) (s) is-

    A
    `-855.4`
    B
    `-673.9`
    C
    `-986.6`
    D
    `-731.7`

  • H_(2)O(l)toH^(+)(aq)+OH^(-)(aq),DeltaH^(0)=57.32kJ*mol^(-1) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),DeltaH^(0)=-285.8kJ*mol^(-1) at 25^(@)C . If DeltaH_(f)^(0)[H^(+)(aq)]=0 , then the standard heat of formation (kJ*mol^(-1)) for OH^(-)(aq) at 25^(@)C is-

    A
    `-142.9`
    B
    `-228.48`
    C
    `-343.12`
    D
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