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Brilliant_brown [7]
3 years ago
9

What would happen to the following endothermic reaction that is in equilibrium if heat is added? N2O4 (g) Two arrows stacked on

top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NO2 (g):
1) The reaction would not be affected

2) The equilibrium would shift to the left

3) The equilibrium would shift to the right

4) The product concentration would equal the reactants
Chemistry
2 answers:
ludmilkaskok [199]3 years ago
7 0
<span>The event that will happen to the following endothermic reaction that is in equilibrium if heat is added is that </span><span>The equilibrium would shift to the right. The correct answer from your choices is number 3.</span>
Ber [7]3 years ago
6 0
The reaction N2O4 (g) <--> 2NO2 (g) is endothermic, meaning that it consumes heat to move towards formation of the products.
According to Le Chatelier's Principle, therefore, if heat is added, more product (NO2) will be produced, and equilibrium would shift towards the right side. This is choice 3.
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A sample of xenon gas occupies a volume of 6.80 L at 52.0°C and 1.05 atm. If it is desired to increase the volume of the gas sam
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Answer:

207.03°C

Explanation:

The following data were obtained from the question:

V1 (initial volume) = 6.80 L

T1 (initial temperature) = 52.0°C = 52 + 273 = 325K

P1 (initial pressure) = 1.05 atm

V2 (final volume) = 7.87 L

P2 (final pressure) = 1.34 atm

T2(final temperature) =?

Using the general gas equation P1V1/T1 = P2V2/T2, the final temperature of the gas sample can be obtained as follow:

P1V1/T1 = P2V2/T2

1.05 x 6.8/325 = 1.34 x 7.87/T2

Cross multiply to express in linear form as shown below:

1.05 x 6.8 x T2 = 325 x 1.34 x 7.87

Divide both side by 1.05 x 6.8

T2 = (325 x 1.34 x 7.87) /(1.05 x 6.8)

T2 = 480.03K

Now, let us convert 480.03K to a number in celsius scale. This is illustrated below:

°C = K - 273

°C = 480.03 - 273

°C = 207.03°C

Therefore, the final temperature of the gas will be 207.03°C

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