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Determine enthalpy of formation for H(2)...

Determine enthalpy of formation for `H_(2)O_(2)(l)`, using listed enthalpies of reaction :
`N_(2)H_(4)(l)+2H_(2)O_(2)(l)rarrN_(2)(g)+4H_(2)O(l), " "Delta_(r )H_(1)^(@)=-818" kJ"//"mol"`
`N_(2)H_(4)(l)+O_(2)(g)rarrN_(2)(g)+2H_(2)O(l)," "Delta_(r )H_(2)^(@)=-622 " kJ"//"mol"`
`H_(2)(g)+1//2O_(2)(g)rarrH_(2)O(l)" "Delta_(r )H_(3)^(@)=-285" kJ"//"mol"`

A

`-383 KJ//"mol"`

B

`-187 KJ//"mol"`

C

`-498 KJ//"mol"`

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
B
For `H_(2)(g) + O_(2)(g) rarr H_(2)O_(2)(l)`
`Delta_(f)H^(@)(H_(2)O_(2),l) = Delta_(r)H_(3)^(@) + (DeltarH_(2)^(@))/(2) - (DeltarH_(1)^(@))/(2)`
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Determine enthalpy of formation for H_(2)O_(2)(l) , using the listed enthalpies of reaction : N_(2)H_(4)(l)+2H_(2)O_(2)(l)toN_(2)(g)+4H_(2)O(l) , " "Delta_(r)H_(1)^(@)=-818kJ//mol N_(2)H_(4)(l)+O_(2)(g)toN_(2)(g)+2H_(2)O(l) " "Delta_(r)H_(2)^(@)=-622kJ//mol H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l)" "Delta_(r)H_(3)^(@)=-285kJ//mol

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Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: CH_(3)OH(l)+3/2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l), …(i), Delta_(r)H_(1)^(Θ)=-726 kJ mol^(-1) C(g)+O_(2)(g) rarr CO_(2)(g), …(ii), Delta_(c )H_(2)^(Θ)=-393 kJ mol^(-1) H_(2)(g)+1/2O_(2)(g) rarr H_(2)O(l), ...(iii), Delta_(f)H_(3)^(Θ)=-286 kJ mol^(-1)

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Compounds with carbon-carbon double bond, such as ethylene, C_(2)H_(4) , add hydrogen in a reaction called hydrogenation. C_(2)H_(4)(g)+H_(2)(g) rarr C_(2)H_(6)(g) Calculate enthalpy change for the reaction, using the following combustion data C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(g) , Delta_("comb")H^(Θ) = -1401 kJ mol^(-1) C_(2)H_(6)(g) + 7//2O_(2)(g)rarr 2CO_(2) (g) + 3H_(2)O(l) , Delta_("comb")H^(Θ) = -1550kJ H_(2)(g) + 1//2O_(2)(g) rarr H_(2)O(l) , Delta_("comb")H^(Θ) = -286.0 kJ mol^(-1)

H_(2)(g)+(1)/(2)O_(2)(g)rarrH_(2)O(l), DeltaH =- 286 kJ 2H_(2)(g)+O_(2)(g)rarr2H_(2)O(l)……………kJ(+-?)

Determine Delta U^(@) at 300K for the following reaction using the listed enthalpies of reaction : 4CO(g)+8H_(2)(g)to3CH_(4)(g)+CO_(2)(g)+2H_(2)O(l) C("graphite")+(1)/(2)O_(2)(g)to CO(g), DeltaH_(1)^(@)=-110.5KJ CO(g)(1)/(2)O_(2)(g)toCO_(2)(g), DeltaH_(2)^(@)=-282.9KJ H_(2)(g)+(1)/(2)O_(2)(g)to H_(2)O(l), DeltaH_(3)^(@)=-285.8KJ C("graphite")+2H_(2)(g)to CH_(4)(g), DeltaH_(4)^(@)=-74.8KJ

Substances that are oxidized and reduced in the following reaction are respectively. N_(2)H_(4)(l)+2H_(2)O_((l))rarrN_(2(g))+4H_(2)O_((l))

Heat of formation of CH_(4) are: If given heat: C(s)+ O_(2)(g) rarr CO_(2) (g) " "DeltaH =-394 KJ 2H_(2) (g)+ O_(2)(g) rarr 2H_(2)O(l) rarr 2H_(2)O(l) " "DeltaH =-568 KJ CH_(4)(g) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l) " " DeltaH =- 892 KJ

For the reaction : C_(2)H_(5)OH(l)+3O_(2)(g)rarr2CO_(2)(g)+3H_(2)O(g) if Delta U^(@)= -1373 kJ mol^(-1) at 298 K . Calculate Delta H^(@)

RESONANCE ENGLISH-THERMODYNAMICS-exercise-3 part-2 Advanced level Solutions
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