Asked by ami

Consider the following equilibrium:



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
Answered by DrBob222
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.
Answered by ami
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
Answered by DrBob222
PCL5(g)=PCL3(g)+CL2(g)

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