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nataly862011 [7]
3 years ago
5

For the same mixture, under the same conditions described in problem 7, calculate keq for 2nh3 (g) n2 (g) + 3h2(g). how is the k

eq for a forward reaction related to the keq for a reverse reaction
Chemistry
1 answer:
nekit [7.7K]3 years ago
7 0

<u>Answer:</u> The relation between the forward and reverse reaction is K_f=\frac{1}{K_r}

<u>Explanation:</u>

For the given chemical equation:

2NH_3(g)\rightleftharpoons N_2 (g)+3H_2(g)

The expression of equilibrium constant for above equation follows:

K_f=\frac{[N_2][H_2]^3}{[NH_3]^2}         .......(1)

The reverse equation follows:

N_2 (g)+3H_2(g)\rightleftharpoons 2NH_3(g)

The expression of equilibrium constant for above equation follows:

K_r=\frac{[NH_3]^2}{[N_2][H_2]^3}       .......(2)

Relation expression 1 and expression 2, we get:

K_f=\frac{1}{K_r}

Hence, the relation between the forward and reverse reaction is K_f=\frac{1}{K_r}

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6 0
2 years ago
if 0.40 mol of h2 and .15 mol of o2 were to reat as completely as possible to produce h20, what mass of the reactant would remai
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Answer:

0.2g

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Number of moles of H₂  = 0.4mol

Number of moles of O₂  = 0.15mol

Unknown:

Mass of reactant that would remain = ?

Solution:

To solve this problem, we need to know the limiting reactant which is the one in short supply in the given reaction.

  The expression of the reaction is :

                2H₂  + O₂  →   2H₂O

                    2 mole of H₂ will combine with 1 mole of O₂

But given;    0.4 mole of H₂ we will require \frac{0.4}{2}  = 0.2mole of O₂

The given number of oxygen gas is 0.15mole and it is the limiting reactant.

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       1 mole of oxygen gas will combine with 2 mole of hydrogen gas

    0.15 mole of oxygen gas will require 0.15 x 2  = 0.3mole of hydrogen gas

Now, the excess mole of hydrogen gas  = 0.4 mole  - 0.3 mole  = 0.1mole

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   Mass of hydrogen gas  = 0.1 x 2 = 0.2g

8 0
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