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Tcecarenko [31]
3 years ago
12

A sample of hydrogen gas at a pressure of 0.926 atm and a temperature of 29.5 C, occupies a volume of 457 mL. If the gas is allo

wed to expand at constant temperature until its pressure is 0.447 atm, the volume of the gas sample will be ___ mL.
Chemistry
1 answer:
klio [65]3 years ago
4 0

Answer:

V₂ = 946.72 mL

Explanation:

Given data;

Initial pressure = 0.926 atm

Initial volume = 457 mL

Temperature = constant = 29.5°C

Final pressure = 0.447 atm

Final volume = ?

Solution:

The given problem will be solved through the Boyle's law,

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume  

by putting values,

P₁V₁ = P₂V₂

0.926 atm × 457 mL = 0.447 atm × V₂

V₂ = 423.18 atm. mL/ 0.447 atm

V₂ = 946.72 mL

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Answer:

The value of the equilibrium constant KC is 1.244

Explanation:

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.550 M, [B] = 1.40 M, and [C] = 0.600 M. The following reaction occurs and equilibrium is established: A+2B<->C

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Step 1: The balanced equation

A+2B<->C

Step 2: The initial concentrations

[A] = 0.550 M

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[C] = 0.600 M

Step 3: The concentraions at equilibrium

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[B]= 1.40 -2X M

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X = 0.120 M

[A] = 0.550 - 0.120 = 0.430 M

[B]= 1.40 -2*0.120 =  1.16 M

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Kc = [C] / [A][B]²

Kc = 0.720 / (0.430*1.16²)

Kc = 1.244

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