Consider a balloon that has a volume V. It contains n moles of gas, it has an internal pressure of P, and its temperature is T.
2 answers:
Answer: The temperature will not change and will remain T.
Explanation: Accoding to ideal gas law:
where,
P = pressure of the gas
V = volume of the gas
T = temperature of the gas
n = number of moles of gas
R = Gas constant = 0.0821 Latm/moleK
= initial pressure
= initial volume
= initial temperature
= final pressure
= final volume
= final temperature
Putting in the values:
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Answer:
Kp = 0.022
Explanation:
<em>Full question: ...With 2.3 atm of ammonia gas at 32. °C. He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 0.69 atm. </em>
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The equilibrium of ammonia occurs as follows:
2NH₃(g) ⇄ N₂(g) + 3H₂(g)
Where Kp is defined as:
<em>Where P represents partial pressure of each gas.</em>
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As initial pressure of ammonia is 2.3atm, its equilibrium concentration will be:
P(NH₃) = 2.3atm - 2X
<em>Where X represents reaction coordinate</em>
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Thus, pressure of hydrogen and nitrogen is:
P(N₂) = X
P(H₂) = 3X.
As partial pressure of hydrogen is 0.69atm:
3X = 0.69
X = 0.23atm:
P(NH₃) = 2.3atm - 2(0.23atm) = 1.84atm
P(N₂) = 0.23atm
P(H₂) = 0.69atm