Judge the spontaneity of the following reaction at 298 K temperature and at a particular pressure:
`Br_2(1) + Cl_2 (g) rarr 2BrCl (g)`.
Given : `Delta H = 29.3 kJ mol^(-1) and Delta S = 104.1 JK^(-1) mol^(-1)`

(i) State Hess's law. (ii) Judge the spontaneity of the following reaction at 298K temperature and at a particular pressure: Br_(2)(l)+Cl_(2)(g)to2BrCl(g) Given: DeltaH=29.3kJ*mol^(-1) and DeltaS=104.1J*K^(-1)*mol^(-1) .

Cl_2(g)rarr 2Cl(g) Delta H^@=242KJ mol^(-1) what is its enthalpy of atomization?

The temperature at which the reaction will be spontaneous C + O_2 = CO_2 , Delta H = 170 kJ mol^-1 , DeltaS = 170 J K^(-1) mol^(-1)

for the reaction 2Cl(g)rarr Cl_2(g) What are the signs of Delta H and Delta S ?

Calculate the value of standard reaction enthalpy for the following reaction : C_2H_5Cl (g) rarr C_2H_4 (g) + HCl (g) at 298 K temperature.Given that DeltaH^@ (C-H) = 413 KJ mol^-1, DeltaH^@ (C-C) = 346 KJ mol^-1 ,DeltaH^@ (C=H) =611 KJ mol^-1, DeltaH^@ (C-CI) = 339 KJ mol^-1 DeltaH^@ (H-Cl) = 432 KJ- mol^-1 .

Br_(2)(l)+Cl_(2)(g)to2BrCl(g) , Whether the reaction is spontaneous or not at a certain pressure & 298 K? [DeltaH=29.3kJ*mol^(-1),DeltaS=104.1J*K^(-1)*mol^(-1)]

Calculate the molar entropy of vaporisation of water , (Given : H_(2)O (l) hArr H_(2)O (g) , Delta H = 40.8 kJ* mol^(-1) )

Is the vaporisation of water at 50^(@)C and 1 atm spontaneous? Given: For vaporisation of water at what temperature and pressure, DeltaH=40.67kJ*mol^(-1) and DeltaS=108.79J*K^(-1)*mol^(-1) .

Calculate the temperature at which DeltaG = -5.2 kJ mol^-1, DeltaH = 145.6 kJ mol^-1 and DeltaS = 216 J K^-1 mol^-1 for a chemical reaction

For a particular reaction, triangleH^@ = -38.3 kJ mol^-1 and triangleS^@ = -113JK^-1 mol^-1 . This reaction is