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1. Predict the sign of ∆S for the reaction, NH3(g) + HCl(g) → NH4Cl(s) 2. The reaction between gaseous hydrogen and chlorine is H2(g) + Cl2(g) → 2HCl(g); ∆rH = -1840 kJ (i) What is the enthalpy of formation of HCl? (ii) How much heat will be liberated at 298 K and 1 atm for the formation of 365 g of HCl? |
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Answer» 1. ∆S is negative 2. (i) ∆fH = \(\frac{-1840}{2}\) = -920 kJ mol-1 (ii) Heat liberated during the formation of 1 mole (36.5 g) of HCl = 920 kJ ∴ Heat liberated during the formation of 365 g of HCl = 9200 kJ |
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