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alexandr402 [8]
3 years ago
11

An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2. At this temperature, Kc

equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g)⇌2 CO2(g). What is the equilibrium concentration of CO?
A) 7.1 × 10-7 M.
B) 8.4 × 10-4 M.
C) 1.4 × 10-2 M.
D) 1.2 × 10-1 M.
Chemistry
2 answers:
Naya [18.7K]3 years ago
8 0
The correct answer to this question is letter "B) 8.4 × 10-4 M."

2CO+O2<->2CO2

-x       -x        +x

It started as 2CO2 so +x, then it decomposed into 2CO and O2, so-x

2CO-oxidized, O2-Oxidized, 2CO2-reduced


the easiest way is to look at the equation, so if we have some reactant and no product 

A<->2C+D

-x    +2x +x
so if we had product concentration, and no reactant concentration 3A<-> C+D +3x -x-x <span>
</span>
salantis [7]3 years ago
5 0

<u>Answer:</u> The correct answer is Option B.

<u>Explanation:</u>

Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as K_{c}

The given chemical reaction follows:

2CO(g)+O_2(g)\rightleftharpoons 2CO_2(g)

The expression of K_{c for above reaction is:

K_c=\frac{[CO_2]^2}{[CO]^2[O_2]}

We are given:

K_c=1.4\times 10^2

[CO_2]=0.0010M

[O_2]=0.0100M

Putting values in above equation, we get:

1.4\times 10^2=\frac{(0.0010)^2}{[CO]^2\times (0.0100)}

[CO]=\sqrt{\frac{(0.0010)^2}{0.0100\times 1.4\times 10^2}}

[CO]=8.4\times 10^{-4}M

Hence, the correct answer is Option B.

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Compare 1 mole of H2, 1 mole of O2, and 1 mole of F2. (a) Which has the largest number of molecules? Explain why. (b) Which has
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<u>Explanation:</u>

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ivanzaharov [21]

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More on stoichiometric calculations can be found here: brainly.com/question/8062886

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2 years ago
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