Standard entropy of `X_2,Y_2 and XY_3` are 60,40, and `50jk^(-1)mol^(-1)` respectively for the reaction `1/2X_2+3/2Y_2 rarr XY_3,Delta H=-30 KJ` what will be the temperature at equilibrium?

Standard entropy of X_(2),Y_(2) and XY_(3) are 60, 40 and 50J*K^(-1)*mol^(-1) respectively. For the reaction (1)/(2)X_(2)+(3)/(2)Y_(2) to XY_(3), (DeltaH=-30kJ) to be at equilibrium, the temperature will be-

In the reaction 1/2N_(2(g)) + 3/2 H_(2(g)) to NH_(3(g)) . The standard entropies of N_(2(g)), H_(2(g)) and NH_(3(g)) are 191.6,130.5 and 192.5 JK^(-1) "mol"^(-1) respectivly. If free energy charge of the reaction is -16.67 kJ. Calculate the Delta H_("reaction")^@ for the formation of NH_3 at 298 K.

If the standard formation enthalpy of CS_2, CO_2 and SO_2 are 117 kJ mol^(-1) -393 kJ mol^(-1) and -297 kJ mol^(-1) respectively then calculate the standard reaction enthalpy of the reaction- CS_2 + 30_2 rarr CO_2 2SO_3 .

The bond dissociation energies of XY, X_2 and Y_2 (all diatomic molecules) are in the reaction 1:1:0:5 and Delta H_r for the formation of XY is -200 KJ mol^(-1) what will be the bond dissociation energy of X_2 ?

For the following reaction at 298K 2X + Y rarr Z DeltaH = 300 kj mol (-1) and DeltaS = 0.2 kj K^(-1) mol^(-1) At what tempreature will the reaction become spontaneous considering Delta H and DeltaS to be constnt over the temperature range?

If the standard formation- enthalpy of CS_(2) , CO_(2) and SO_(2) are 117 kJ * mol^(-1) , -393 kJ * mol^(-1) and -297 kJ * mol^(-1) respectively , calculate the standard reaction enthalpy of - CS_(2) + 3O_(2) to CO_(2) + 2 SO_(2)

(i) State hess's law. (ii) For the following reaction at 298K 2X+Y to Z DeltaH=300kJ*mol^(-1) and DeltaS=0.2kJ*K^(-1)*mol^(-1) At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?

If x:y = 5:7 what will be 1/x^2: 1/y^2 ?

Factorise : (x^(2)-1)(y^(2)-1)-4xy