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3 years ago

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A sample of carbon dioxide occupies a volume of 2.50 liters at 100 kPa pressure. What pressure would the gas exert if the volume

was decreased to .75 liters? Round two decimal places.

1 answer:

ira [324]3 years ago

4 0

Answer:

333.33 KPa

Explanation:

P1V1=P2V2

p2=P1v1/v2

p2= (2.50 L* 100 kPa)/0.75 L

P2=333.33 kPa

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Gas in a balloon occupies 3.3 L. What volume will it occupy if the pressure is changed from 100.0 kPa to 90.0 kPa (at constant t

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Since the temperature is a constant, we can use Boyle's law to solve this.<span>

<span>Boyle' law says "at a constant temperature, the pressure of a fixed amount of an ideal gas is inversely proportional to its volume.

P α 1/V </span>⇒ PV = k (constant)<span>

Where, P is the pressure of the gas and V is the volume.

<span>Here, we assume that the </span>gas in the balloon is an ideal gas.

We can use Boyle's law for these two situations as,
P</span>₁V₁ = P₂V₂<span>

P₁ = 100.0 kPa = 1 x 10⁵ Pa
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By substitution,
1 x 10⁵ Pa x 3.3 L = 90 x 10³ Pa x V₂</span><span>
V</span>₂ = 3.7 L<span>
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Explanation:

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is correct answer

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mars1129 [50]

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2 HI(g) ⇄ H2(g) + I2(g) Kc = 0.0156 at 400ºC 0.550 moles of HI are placed in a 2.00 L container and the system is allowed to rea

Alex_Xolod [135]

<u>Answer:</u> The concentration of hydrogen gas at equilibrium is 0.0275 M

<u>Explanation:</u>

Molarity is calculated by using the equation:

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For the given chemical equation:

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<u>At eqllm:</u> 0.275-2x x x

The expression of $K_c$ for above equation follows:

$K_c=\frac{[H_2][I_2]}{[HI]^2}$

We are given:

$K_c=0.0156$

Putting values in above expression, we get:

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