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Alborosie
3 years ago
10

Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g) K=0.042 The concentrations of the products at equilibrium are [PCl3]=0.18 M and

[Cl2]=0.30 M . What is the concentration of the reactant, PCl5, at equilibrium?
Chemistry
1 answer:
tatyana61 [14]3 years ago
6 0

<u>Answer:</u> The equilibrium concentration of PCl_5 is 1.285 M.

<u>Explanation:</u>

The chemical equation for the decomposition of phosphorus pentachloride follows:

PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)

The expression for equilibrium constant is given as:

K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}

We are given:

K_c=0.042

[PCl_3]=0.18M

[Cl_2]=0.30M

The concentration of solid substances are taken to be 1. Thus, they do not appear in the equilibrium constant expression.

Putting values in above equation, we get:

0.042=\frac{0.18\times 0.30}{[PCl_5]}

[PCl_5]=1.285

Hence, the equilibrium concentration of PCl_5 is 1.285 M.

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The molar mass of uranium-235 is 235 g/mol. So one mole of uranium-235 has a mass of 235 g. Put differently 6.022×10^23 atoms of uranium-235 have a mass of 235 g. Knowing that, how can we use that to find the mass of one atom?

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3 years ago
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The rate of disappearance of NO = -\frac{1}{2}\frac{d[NO]}{dt}

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The rate of formation of NOCl = \frac{1}{2}\frac{d[NOCl]}{dt}

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