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maria [59]
3 years ago
6

How many liters of ammonia are required to change 34.9 L of nitrogen monoxide to nitrogen gas? Assume 100% yield and that all ga

ses are measured at the same temperature and pressure.
Chemistry
1 answer:
frutty [35]3 years ago
4 0

Answer:

23.27 L

Explanation:

The balanced reaction of ammonia and nitrogen monoxide is shown below as:

4NH₃(g) + 6NO(g) ⇒ 5N₂(g) + 6H₂O(l)

Given that:

Volume of nitrogen monoxide = 34.9 L

Since, temperature and pressure are same, volume coefficients would be same as equation coefficients.

So,

6 L of nitrogen monoxide reacts with 4 L of ammonia.

1 L of nitrogen monoxide reacts with 4/6 L of ammonia.

34.9 L of nitrogen monoxide reacts with (4/6)*34.9 L of ammonia.

Amount of ammonia required = 23.27 L

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2) Assuming that when the valve is opened there is not change in temperature, there will be 1.00 + 2.00 moles of gas in a volumen of 2 liters.

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which compared to the initial pressure in chamber 1, p1, is:

p / p1 = (3/2) / 2 = 3/4 => p = (3/4)p1

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p / p2 = (3/2) / 1 = 3/2, which means that the pressure in the chamber 2 decreases to 3/2 of its original pressure.
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