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
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.
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
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.
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
To determine how many moles of Cl2 are present at equilibrium, we need to consider the balanced equation for the reaction and use the given information.
The balanced equation for the reaction is:
Cl2 ⇌ 2Cl
From the equation, we can see that 1 mole of Cl2 produces 2 moles of Cl. So, if 1.0 mole of Cl is present at equilibrium, we can conclude that 0.5 moles of Cl2 will be present (since 1 mole of Cl is produced for every 0.5 moles of Cl2).
Therefore, the correct answer is option a. 0 moles of Cl2 are present at equilibrium.