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serg [7]
2 years ago
9

In a reaction where A + B AB, what does an equilibrium position of A= 14%, B = 14%, and AB= 72% indicate about the reaction?

Chemistry
2 answers:
MissTica2 years ago
5 0
The answer is c I just answered mine .
fomenos2 years ago
3 0
<span>A.) Because A and B are equal, the reaction has reached equilibrium.
B.) There is more A and B than AB at equilibrium, and the reaction favors the reactants.
C.) There is more AB than A and B at equilibrium, and the reaction favors the products.
D.) There is more AB than A and B at equilibrium, and the reaction favors the reactants.
E.) The reaction is not at equilibrium. 
These are the answer choices pls help
</span>
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exis [7]

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70 mL of 5% HCl and 30 mL of 15% HCl

Explanation:

We will designate x to be the fraction of the final solution that is composed of 5% HCl, and y to be the fraction of the final solution that is composed of 15% HCl. Since the percentage of the final solution is 8%, we can write the following expression:

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Since x and y are fractions of a total, they must equal one:

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This is a system of two equations with two unknowns. We will proceed to solve for x. First, an expression for y is found:

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This expression is substituted into the first equation and we solve for x.

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(100 mL)(0.7) = 70 mL

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