Question

In: Chemistry

Consider the following reaction:  2 A + 3 B2 ⇌ A2B6 The initial concentrations of...

Consider the following reaction:  2 A + 3 B2 ⇌ A2B6

The initial concentrations of A and B2 are 0.245 M and 0.730 M, respectively, with no A2B6 initially present. When the reaction comes to equilibrium, the concentration of A2B6 is found to be 9.50×10−2 M.

Part A

What is the equilibrium concentration of A?

Round your answer to 3 significant figures.

Part B

What is the equilibrium concentration of B2?

Round your answer to 3 significant figures.

Part C

What is the value of the equilibrium constant?

Round you answer to 3 significant figures.

Solutions

Expert Solution

The easiest approach for calculating equilibrium concentrations is to use an ICE Table, which is an organized method to track which quantities are known and which need to be calculated. ICE stands for:

"I" is for the "initial" concentration or the initial amount
"C" is for the "change" in concentration or change in the amount from the initial state to equilibrium
"E" is for the "equilibrium" concentration or amount and represents the expression for the amounts at equilibrium.

the concentration for the reactant are added to the initial row of the table. the iniital amount of A2H6 is not given, so it is given a value of 0.

                             2 A                       B                               A2B6

Initial                     0.245 M               0.730M                      0

Change                 2* 0.245 - 9.50*10-2M          3* 0.730 - 9.50*10-2M               9.50*10-2M

Equilibrium               0.395                                2.095                             9.50*10-2M

queen_honey_blossom answered 2 years ago
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