Calculate the standard free energy change for the reaction,
`N_(2(g))+3H_(2(g))to2NH_(3(g)) at 298 K`.
Given, `DeltaH^@ =-92.4kJ` and `DeltaS^@ = -198.3 JK^(-1)`. Also, comment on the result.

Determine standard free energy DeltaG^@" at " 25^@C for the reaction N_2(g) + 3H_2(g) hArr 2NH_3(g) Given: DeltaH^@ = -91.8 kJ , DeltaS^@ = - 198 J K^(-1)

In the given reaction, calculate the standard free energy change at 25^(@)C:N_(2)(g)+3H_(2)(g)to2NH_(3) [Given that, DeltaH^(0)=-91.8kJ and DeltaS^(0)=-198J*K^(-1) ]

Calculate the free eneryg change at 298 K for the reaction , Br_(2)(l)+Cl_(2)(g) to BrCl(g) . For the reaction DeltaH^(@)=29.3 kJ &

The enthalpy change for the reaction, N_2(g)+3H_2(g)rightarrow2NH_3(g) Is -92.38 kJ at 298 K. What is DeltaU at 298 K?

The enthalpy change for the reaction. N_(2(g))+3H_(2(g))rightarrow2NH_(3(g)) is - 91.8 kJ at 298 K.what is Delta U at 298K? ( R=8.314 JK^-1mol^-1 )

What will be the standard internal energy change for the reaction at 298 K ? OF_(2(g))+H_(2)O_((g))rarr 2HF_((g)) +O_(2)(g) ,DeltaH^(@)=-310kJ

Calculate the standard free energy change for the following reaction at 27^@C . H_2(g) + I_2(g) to 2HI(g) , DeltaH^@ = + 51.9 kJ [Given : DeltaS_(H_2)^@ = 130.6 JK^(-1) mol^(-1) DeltaS_(I_2)^@ = 116.7 JK^(-1) mol^(-1) DeltaS_(HI)^@ = 206.3 JK^(-1) mol^(-1)] . Predict whether the reaction is feasible at 27°C or not.

For reaction, N_(2(g))+3H_(2(g))to2NH_(3(g)) , DeltaH=-95.4kJ and DeltaS=-198.3JK^(-1) . Calculate the maximum temperature at which the reaction will proceed in forward direction.

The enthaply change (Delta H) for reaction, N_(2) (g) + 3H_(2)(g) to 2NH_(3) (g) is 92.38 kj at 298 K. What is Delta U at 298 K ?