For formation of ammonia `Delta H=-46(kJ)/(mol)`, `Delta S=-198(J)/(mol.K)` , then the reaction is at equilibrium at temperature `100x`. What is value of `x` if it is rounded off to nearest two digit number.

If a process has Delta H = 548.3 kJ and Delta S = 32 J/mole at 298 K then will the process be spontaneous at this temperature ?

For a given reaction, DeltaH = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol^(-1) . The reaction is spontaneous at (Assume that DeltaH and DeltaS do not vary with temperature)

For a given reaction, Delta H = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol(-1) . The reaction is spontaneous at : (Assume that Delta H and Delta S do not vary with temperature)

It is planned to carry out the reaction: CaCO_(3)(s) hArr CaO(s) +CO_(2)(g) at 1273K and 1 bar pressure. Delta_(r)G^(Theta) = 176 kJ mol^(-1) and Delta_(r)S^(Theta) = 157.2 kJ mol^(-1) a. Is the reaction spontaneous at this temperature and pressure ? b. Calculate the value of i. K_(p) at 1273K for the reaction ii. partial pressure of CO_(2) at equilibrium

A process has Delta H= 200 J mol^(-1) and DeltaS=40" JK"^(-1)mol^(-1) . Out of the values given below, choose the minimum temperature above which the process will be spontaneous :

For the reaction at 300 K A(g)hArrV(g)+S(g) Delta_(r)H^(@)=-30kJ//mol, Delta_(r)S^(@)=-0.1kJK^(-1).mol^(-1) What is the value of equilibrium constant ?

A certain reaction is at equilbrium at 82^(@)C and Delta H for this reaction is 21.3 kJ. What would be the value of Delta S (in JK^(-1)mol^(1) ) for the reaction?

For a hypothetical reaction A(g) + 3B(g) to 2C(g). Delta H = -100 kJ and Delta S = -200 Jk^(-1) . Then the temperature at which the reaction will be in equilibrium is

Delta_(vap)H = 30 kJ mol^(-1) and Delta_(vap)S = 75Jmol^(-1)K^(-1) . Find the temperature of vapour, at 1 atm.

The Delta S for the vaporisation of 1 mol of water is 88.3 J/mole K. The value of Delta S for the condensation of 1 mole of water vapour will be