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H(2)(g) +CI(2)(g) rarr 2HCI(g) +185 kJ. ...

`H_(2)(g) +CI_(2)(g) rarr 2HCI(g) +185 kJ`. State whether this reaction is exo or endothermic and why?

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It is an expthermic reaction because heat is being evolved.
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H_(2) (g) +I_(2) (g) rarr 2HI (g), DeltaH=51.9 kJ . According to this, heat of formation of HI is

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For the reactions, N_(2)(g) +3H_(2)(g) rarr 2NH_(3)(g) predict, whether the work is done on the system or by the system.

Compounds with carbon-carbon double bond, such as ethylene, C_(2)H_(4) , add hydrogen in a reaction called hydrogenation. C_(2)H_(4)(g)+H_(2)(g) rarr C_(2)H_(6)(g) Calculate enthalpy change for the reaction, using the following combustion data C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(g) , Delta_("comb")H^(Θ) = -1401 kJ mol^(-1) C_(2)H_(6)(g) + 7//2O_(2)(g)rarr 2CO_(2) (g) + 3H_(2)O(l) , Delta_("comb")H^(Θ) = -1550kJ H_(2)(g) + 1//2O_(2)(g) rarr H_(2)O(l) , Delta_("comb")H^(Θ) = -286.0 kJ mol^(-1)

The reaction between gaseous hydrogen and chlorine is H_(2)(g) + CI_(2)(g) to 2HCI(g) Delta_(r)H^(@) = -184.0 kJ (i) What is the enthalpy of formation of HCI? How much heat will be liberated at 298 K and 1 atm for the formation of 365 g of HCI?

H_(2)(g)+I_(2)(g)rArr2HI(g) (DeltaH=+51.8KH=KJ] What is the equilibrium constant expression for this system?

CENGAGE CHEMISTRY-THERMODYNAMICS-Exercises (Subjective)
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