For the following reaction scheme, percentage yields are given along the arrow:


x g and y g are mass of R and U, respectively.

(Use : Molar mass (in g mol^$$-$$1) of H, C and O as 1, 12 and 16, respectively)

The value of y is ________.

For the reaction, X(s) $$\rightleftharpoons$$ Y(s) + Z(g), the plot of $$\ln {{pz} \over {{p^\theta }}}$$ versus $${{{{10}^4}} \over T}$$ is given below (in solid line), where p_z is the pressure (in bar) of the gas Z at temperature T and $${{p^\theta }}$$ = 1 bar.


(Given, $${{d(\ln K)} \over {d\left( {{1 \over T}} \right)}} = - {{\Delta {H^\theta }} \over R}$$, where the equilibrium
constant, $$K = {{pz} \over {{p^\theta }}}$$ and the gas constant, R = 8.314 J K^$$-$$1 mol^$$-$$1)

The value of standard enthalpy, $$\Delta$$H^o (in kJ mol^$$-$$1) for the given reaction is _______.

For the reaction, X(s) $$\rightleftharpoons$$ Y(s) + Z(g), the plot of $$\ln {{pz} \over {{p^\theta }}}$$ versus $${{{{10}^4}} \over T}$$ is given below (in solid line), where p_z is the pressure (in bar) of the gas Z at temperature T and $${{p^\theta }}$$ = 1 bar.


(Given, $${{d(\ln K)} \over {d\left( {{1 \over T}} \right)}} = - {{\Delta {H^\theta }} \over R}$$, where the equilibrium
constant, $$K = {{pz} \over {{p^\theta }}}$$ and the gas constant, R = 8.314 J K^$$-$$1 mol^$$-$$1)

The value of $$\Delta$$S^$$\theta$$ (in J K^$$-$$1 mol^$$-$$1) for the given reaction, at 1000 K is _________.

The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x$$^\circ$$C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y $$\times$$ 10^$$-$$2$$^\circ$$C.

(Assume : Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.

Use : Molal elevation constant (Ebullioscopic Constant), K_b = 0.5 K kg mol^$$-$$1; Boiling point of pure water as 100$$^\circ$$C.)

The value of x is ________.