Enthalpy 1

Chemistry Level 2

Red phosphorus reacts with liquid bromine in the following exothermic reaction:

2 P ( s ) + 3 Br 2 ( l ) → 2 PBr 3 ( g ) , Δ H = − 243.0 kJ 2 \text{P}(s) +3 \text{Br}_{2}(l) \rightarrow 2 \text{PBr}_{3}(g),\qquad\Delta H=-243.0\text{ kJ}

Calculate the enthalpy change when 5.26 5.26 g phosphorus reacts with an excess amount of bromine.

− 20.60 kJ -20.60\text{ kJ} − 15.50 kJ -15.50\text{ kJ} − 10.30 kJ -10.30\text{ kJ} − 5.15 kJ -5.15\text{ kJ}

Krishna Singh by Krishna Singh , 22, India

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