`DeltaH^@` & `DeltaS^@` for the reaction `H_2 (g) + I_2 (g) = 2 HI (g) are 16.23 Kj mol^-1` and `63.8 kj mol^-1` predic whether the reaction be spontaneous at `35^@C`.

For the reaction at 298 k,2A +B rarr C, Delta H= 400 KJ mol^(-1) and Delta S=0.2 KJ k^(-1) mol^(-1). At what temperature will the reaction become spontaneous ?

The values of DeltaH and DeltaS of a certain reaction are -400 kJ mol^-1 and -20 kJ mol^-1 respectively. The temperature below which the reaction is spontaneous is

DeltaH and DeltaS of a certain reaction are -400 kJ*mol^(-1) and -20kJ*mol^(-1)*K^(-1) respectively. The temperature below which the reaction is spontaneous is-

For the reaction between CO_2 and graphite CO_2(g)+C(s)rarr 2CO(g) , DeltaH=+170KJ and Delta S=170JK^(-1) the reaction is spontaneous at

Values of Delta H Delta S for the given reaction are -95.4 kJ and -198.3 J*K^(-1) respectively: N_(2)(g)+3H_(2)(g) to 2NH_(3)(g) State whether the reaction will be spontaneous at 500 K or not. Consider Delta H and DeltaS are independent of temperature.

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?

At 448^@C , the equilibrium constant (K_C) for the reaction H_2(g) + I_2(g) iff 2HI(g) is 50.5. Predict the direction in which the reaction will proceed to reach equilibrium at 448^@C , if we start with 2.0 xx 10^-2 mol of HI, 1.0 xx 10^-2 mol of H_2 and 3.0 xx 10^-2 mol of I_2 In a 20L- container.

At 25^(@)C and 1 atm pressure, DeltaH and pressure-volume work for the reaction, 2H_(2)(g)+O_(2)(g)to2H_(2)O(g) , are -483.7kJ and 2.47kJ respectively. In this reaction the value of DeltaU is-

H_(2)(g)+Br_(2)(l) to 2HB r (g),DeltaH=-72.8kJ("1 atm ",25^(@)C) if molar entropies of H_(2)(g),Br_(2)(l),HB r(g) are 130.5, 152. 3 & 198.3 J*K^(-1)*mol^(-1) respectively then at which temperature the reaction will be spontaneous?

(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?