Consider the following equilibrium:

Question

5.0 moles of are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of Cl2 are present at equilibrium.
Choose one answer.

a. 0

b. 1.0

c. 2.0

d. 3.0

e. 4.0

Answer 1

Ami--Are you taunting those trying to help? ;-).
You didn't provide the equilibrium reaction. also look at your first post today. It isn't complete either.

Answer 2

PCL5(g)=PCL3(g)+CL2(g)

5.0 moles of are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of Cl2 are present at equilibrium.
Choose one answer.

a. 0

b. 1.0

c. 2.0

d. 3.0

e. 4.0

Answer 3

PCL5(g)=PCL3(g)+CL2(g)

5.0 moles ofWHAT are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of WHAT is present in the equilibrium mixture. How many moles of Cl2 are present at equilibrium.
Choose one answer.

Answer 4

PCL5(g)=PCL3(g)+CL2(g)

5.0 moles of PCL5 are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of Cl2 are present at equilibrium.
Choose one answer.

a. 0

b. 1.0

c. 2.0

d. 3.0

e. 4.0