For the process
`NH_(3)(g) +HCI(g) rarr NH_(4)CI(s)`

For the process NH_(3)(g) +HCI(g) rarr NH_(4)Cl(s)

Predict DeltaS for the reaction : NH_(3)(g) + HCI (g) to NH_(4)CI(s) .

A 5.00L evacuated cylinder is charged with 25.5g of NH_(3) and 36.4 g of HCl. Calculate the final pressure at 85.0^(@)C after the two compounds have reacted completely: NH_(3)(g)+HCl(g)rarrNH_(4)CI(s)

a) Predict the sign of DeltaS for the reaction, NH_3(g)+HCI(g)rightarrowNH_4CI(s) b) The reaction between gaseous hydrogen and chlorine is H_2(g)+CI_2(g)rightarrow2HCI(g), Delta_rH=-1840 kJ i) What is the enthalpy of formation of HCI? ii) How much heat will be liberated at 298 K and 1 atm for the formation of 365 g of HCI?

If Delta_(f)G^(@) for NH_(3)(g) is - 16.4 kJ mol^(-1) , then Delta G^(@) for the reaction : N_(2)(g) + 3 H_(2)(g) rarr 2NH_(3)(g) is