Home
Class 11
CHEMISTRY
Delta(f)U^(@) of combustion of CH4(g)at ...

`Delta_(f)U^(@)` of combustion of `CH_4(g)`at certain temperature is `-393kJmol^(-1)`.The value of `Delta_(f)H^(@)` is

Promotional Banner

Similar Questions

Explore conceptually related problems

DeltaU^(@) of combustion of CH_(4(g)) at certain temperature is -"393 kJ mol"^(-1) . The value of DeltaH^(@) is

delta_(f) U^(Ó¨) "of formation of" CH_(4)(g) at a certain temperature is -393Jmol^(-1). The value of delta H^(Ó¨)is:

delta H -delta E for the combustion of gaseous propane at temperature T is

Calorific value of H_2 is -143KJ g^(-1) . Hence, Delta H_(f)^(@) of H_2O is:

The enthalpy change for the combustion of N_(2)H_(4)(l) (Hydrazine) is -622.2 kJ mol^(-1) . The products are N_(2)(g) and H_(2)O(l) . If Delta_(f)H^(Theta) for H_(2)O(l) is -285.8 kJ mol^(-1) . The Delta_(f)H^(Theta) for hydrazine is

The value of DeltaE for combustion of 16 g of CH_4 is -885389 at 298 K. The DeltaH combustion for CH_4 in Jmol^(-1) at this temperature will be : (Given that, R = 8.314 JK^(-1) mol^(-1) )

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )H^(@) at 300 K for the reaction is :

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )H^(@) at 320 K is :

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )S^(@) at 300 K for the reaction is :

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )S^(@) at 320 K is :