Multiple Choice
The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) ⇄ 2BrCl(g)
What is the equilibrium constant for the following reaction?
BrCl(g) ⇄ ½Br2(g) + ½Cl2(g)
A) 2.97 × 10 −4
B) 1.72 × 10 −2
C) 3.45 × 10 −2
D) 1.31 × 10 −1
E) > 1.00
Correct Answer:
Verified
Correct Answer:
Verified
Q51: Consider the equilibrium reaction shown below. B<sub>2</sub>(g)
Q52: Consider the reversible reaction: 2NO<sub>2</sub>(g) ⇄ N<sub>2</sub>O<sub>4</sub>(g)
Q53: When a reaction system reaches equilibrium, the
Q54: Write the mass-action expression, Q<sub>c</sub>, for the
Q55: Unless ΔH°<sub>rxn</sub> = 0, a change in
Q57: Consider the equilibrium reaction: H<sub>2</sub>(g) + Br<sub>2</sub>(g)
Q58: At 850°C, the equilibrium constant K<sub>p</sub> for
Q59: Carbon monoxide and chlorine combine in an
Q60: Carbon monoxide and chlorine combine in an
Q61: For some gas-phase reactions, K<sub>p</sub> = K<sub>c</sub>.