Home
Class 12
CHEMISTRY
Consider the reaction below at 298K, C...

Consider the reaction below at 298K,
`C("graphite")+2H_(2)(g) to CH_(4) (G)`
`triangle_(f) H^(@) ("Kj/mol") -74.9`
`S_(m)^(@) ("J/mol-K")+5.6 +130.7 +186.3`
Which statement below is correct?

A

`triangle_(r)G^(@)` is -50.8 kJ and the reaction is driven by enthalpy only

B

`triangle_(r)G^(@)` is -50.8 kJ and the reaction is driven by entropy only

C

`triangle_(r)G^(@)` is +50.8 kJ and the reaction is driven by both enthalpy and entropy

D

`triangle_(r)G^(@)`is -50,8 kJ and the reaction is driven by both enthalpy and entropy

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the standard Gibbs energy change for the formation of propane at 298 K: 3C("graphite") + 4H_(2)(g) to C_(3)H_(8)(g) Delta_(f)H^(@) for propane, C_(3)H_(8)(g) = -103.8 kJ mol^(-1) . Given : S_(m)^(0)[C_(3)H_(8)(g)] = 270.2 J K^(-1) "mol"^(-1) S_(m)^(@)("graphite") = 5.70 J K^(-1) "mol"^(-1) and S_(m)^(0)[H_(2)(g)] = 130.7 J K^(-1) "mol"^(-1) .

Calculate the standard free energy change for the formation of methane at 300K : C("graphite") +2H_(2) (g) rarr CH_(4)(g) The following data are given: Delta_(f)H^(Theta) (kJ mol^(-1)): CH_(4)(g) =- 74.81 Delta_(f)S^(Theta)(kJ mol^(-1)): C("graphite") = 5.70, H_(2)(g) = 130.7 CH_(4)(g) = 186.3

Calculate the standard molar entropy change for the formation of gaseous propane (C_(3)H_(8)) at 293K . 3C("graphite") +4H_(2)(g) rarr C_(3)H_(8)(g) Standard molar entropies S_(m)^(Theta) (JK^(-1)mol^(-1)) are: C("graphite") = 5.7, H_(2)(g) = 130.7,C_(3)H_(5)(g) = 270.2

Calculate the equilibrium constant for the following reaction at 298K and 1 atmospheric pressure: C(graphite) +H_(2)O(l) rarr CO(g) +H_(2)(g) Given Delta_(f)H^(Theta) at 298 K for H_(2)O(l) =- 286.0 kJ mol^(-1) for CO(g) =- 110.5 kJ mol^(-1) DeltaS^(Theta) at 298K for the reaction = 252.6 J K^(-1) mol^(-1)

Consider the following reaction at temperature T : CH_(2)=CH_(2)(g) +Cl_(2)(g)rarrClCH_(2)CH_(2)Cl(g) Delta_(r ) H^(@)=-217.5kJ//"mol, " Delta_(r )S^(@)=-233.9J//K-"mol" Reaction is supported by :

Determine the enthalpy change of the reaction. C_(3)H_(5) (g) + H_(2) (g) rarr C_(2)H_(6) (g) + CH_(4) (g) at 25^(@)C , using the given heat of combustion value under standard conditions: Compound H_(2) (g) CH_(4) (g) C_(2) H_(6) (g) C (graphite) Delta H^(@) (kJ//mol) -285.8 =890.0 - 1560.0 -393.5 The standard heat of formation of C_(3)H_(8) (g) is -103.8 kJ//mol

For the reaction, SO_(2)(g)+1//2O_(2)(g)hArrSO_(3)(g) DeltaH_(298)^(@)=-98.32KJ//mol e,DeltaS_(298)^(@)=-95.0J//mol e-K . Find the K_(p) for this reaction at 298K.