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Evgen [1.6K]
2 years ago
9

Given that Kp [NOTE: Kp!!!!] = 1.39 at 400 ºC for the reaction, P4(g) <=> 2 P2(g), which answer best describes the reactio

n when 2.50 mol of P4(g) and 1.50 mol of P2(g) are mixed in a 25.0 L, closed container at 400 ºC? [REMEMBER: it’s Kp]
Chemistry
1 answer:
Igoryamba2 years ago
3 0

Answer:

The reaction will proceed to the left to attain equilibrium.

Explanation:

The question is missing but I guess it must be about <em>how the reaction will proceed to attain equilibrium.</em>

First, we have to calculate the partial pressures using the ideal gas equation.

pP_{4}=\frac{2.50mol\times (0.08206atm.L/mol.K)\times 673K}{25.0L} =5.52atm

pP_{2}=\frac{1.50mol\times (0.08206atm.L/mol.K)\times 673K}{25.0L}=3.31atm

Now, we have to calculate the reaction quotient (Qp).

Qp=\frac{pP_{2}^{2}}{pP_{4}} =\frac{3.31^{2} }{5.52} =1.98

Since Qp > Kp, the reaction will proceed to the left to attain equilibrium.

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Answer:

c

Explanation:

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2 years ago
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Answer:

c) the overall reaction order is 1.

Explanation:

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creativ13 [48]
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8 0
3 years ago
A helium balloon is filled on the ground where the atmospheric pressure is 768 torr. The volume of the balloon is 8.00 m3. When
Anvisha [2.4K]

Answer:

The correct option is: <u>B. 366 torr</u>

Explanation:

Given: <u>On the ground</u>- Initial Volume: V₁ = 8.00 m³, Initial Atmospheric Pressure: P₁= 768 torr;

<u>At 4200 m height</u>- Final Volume: V₂ = 16.80 m³, Final Atmospheric Pressure: P₂ = ?

Amount of gas: n, and Temperature: T = constant

<u>According to the Boyle's Law</u>, for a given amount of gas at constant temperature:         P₁ V₁ = P₂ V₂

⇒  P₂ = P₁ V₁ ÷ V₂

⇒  P₂ = [(768 torr) × (8.00 m³)] ÷ (16.80 m³)

⇒  P₂ = 365.71 torr ≈ 366 torr

<u>Therefore, the final air pressure at 4200 m height: P₂ = 366 torr.</u>

6 0
3 years ago
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-Dominant- [34]

Answer:

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Explanation:

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5 0
2 years ago
Read 2 more answers
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