Question

question 7 (1 point) saved
when pressure i and volume ii the reaction in an equilibrium system shifts in
the direction that produces iii particles.
the statement given above is completed by the information given in the row:

row	i	ii	iii
b	increases	decreases	more
c	decreases	increases	less
d	decreases	increases	the same number of
e	increases	decreases	the same number of

a
b
c
d
e

Explanation:

To solve this, we use Le Chatelier's principle for gas equilibrium. Pressure and volume are inversely related (for gases, \( P \propto \frac{1}{V} \) at constant temp). When pressure decreases (\( i \)) and volume increases (\( ii \)), the system shifts to produce more particles (to counteract the lower pressure by increasing the number of gas particles, which increases pressure). Let's analyze each row:

• Row A: \( i \)=decreases, \( ii \)=increases, \( iii \)=more. This matches the principle: lower pressure (higher volume) causes equilibrium to shift toward more particles to increase pressure.
• Row B: \( i \)=increases, \( ii \)=decreases would shift to fewer particles (not more), so B is wrong.
• Row C: \( iii \)=less is incorrect (lower pressure needs more particles, not less).
• Row D: \( iii \)=same number is wrong (change in pressure/volume affects particle count direction).
• Row E: \( i \)=increases, \( ii \)=decreases would shift to fewer particles, and \( iii \)=same is wrong.

So Row A is correct.

Answer:

A. decreases, increases, more