4pcl₃(l) p₄(s) + 6cl₂(g); δh= 304.0 kj
based on the reaction shown, which statement is true?
a) when 1 mol pcl₃(l) reacts, 304.0 kj are released. b) when 1 mol p₄(s) is produced, 304.0 kj are consumed. c) when 548.56 g pcl₃(l) react, 304.0 kj are released. d) when 137.14 g pcl₃(l) react, 304.0 kj are consumed. e) when 123.88 g p₄(s) are produced, 304.0 kj are released.

The following statement is true

When 137.14 g PCl₃(l) react, 304.0 kJ are consumed.

Explanation:

The given equation is

Molecular weight of

PCl₃ = 137.14

P₄ = 123.88

The enthalpy is positive which means the reaction is endothermic.

The reaction will absorb energy from the surroundings.

A) When 1 mol PCl₃(l) reacts, 304.0 kJ are released: False, energy is being absorbed not released

B) When 1 mol P₄(s) is produced, 304.0 kJ are consumed: False as the reverse reaction will be exothermic and there will be release of energy during formation of phosphorus.

C) When 548.56 g PCl₃(l) react, 304.0 kJ are released: Energy is being consumed so it is false

D) When 137.14 g PCl₃(l) react, 304.0 kJ are consumed:True as the enthalpy of reaction is 304.0 kJ

E) When 123.88 g P₄(s) are produced, 304.0 kJ are released: Energy is being consumed so the statement is False.

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