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mafiozo [28]
4 years ago
13

The reaction for the synthesis of ammonia N2(g) + 3 H2(g) → 2 NH3(g) is exothermic. Increasing the temperature applied to the sy

stem I) increases the amount of NH3. II) decreases the amount of NH3. III) changes the value of Keq. IV) does not change the value of Keq.
Chemistry
1 answer:
igomit [66]4 years ago
5 0

Answer:

The correct statements are (II) and (III).

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

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

This is a type of exothermic reaction because heat is released in the reaction.

On increasing the temperature

If the temperature is increased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where decrease in temperature occurs. As, this is an exothermic reaction, forward reaction will increase the temperature. Hence, the equilibrium will shift in the left direction.

And by moving to left side amount of ammonia will decrease accompanied by the change in the value of an equilibrium constant.

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FromTheMoon [43]

Answer:

Option 4 is correct (72 seconds)

Explanation:

Option 4 is correct (72 seconds)

The formula we are going to use is:

ln\frac{A}{A_o}=-kt

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A_o is the initial concentration

k is the constant

t is the time

Half-Life=0.693/k

Half-life in our case=24 seconds

k=0.693/24

k=0.028875 s^-1

Since the concentration is decreased by 87.5 % which means only 12.5%(100-87.5%) is left.

The ratio A/A_o will become 0.125

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irina [24]

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Explanation:

Considering:

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Or,

Moles =Molarity \times {Volume\ of\ the\ solution}

Given :

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The conversion of mL to L is shown below:

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