Question

4 PCl₃(l)
`\longrightarrow` 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.

Answer 1

The following statement is true

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

Step-by-step explanation:

The given equation is

`PCl_(3)(l)--->P_(4)(s)+6Cl_(2)`

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.