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gulaghasi [49]
3 years ago
13

At constant temperature, 534 mL of a gas at 894 torr is compressed to 167 mL What is the new pressure in atmospheres?

Chemistry
2 answers:
AURORKA [14]3 years ago
8 0

Answer:

3.762 atm.

Explanation:

  • We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R  is the general gas constant,

T is the temperature of the gas in K.

  • If n and T are constant, and have different values of P and V:

<em>(P₁V₁) = (P₂V₂)</em>

<em></em>

  • Knowing that:

P₁ = 894.0 torr, V₁ = 534.0 mL,

P₂ = ??? torr, V₂ = 167.0 mL.

  • Applying in the above equation

(P₁V₁) = (P₂V₂)

<em>∴ P₂ = (P₁V₁)/V₂</em> = (894.0 torr)(534.0 mL)/(167.0 mL) = <em>2859 torr.</em>

  • To convert from torr to atm:

1.0 atm = 760.0 torr.

<em>∴ P₂ </em>= (2859 torr)(1.0 atm/760 torr) = <em>3.762 atm.</em>

daser333 [38]3 years ago
8 0

Answer:

B)3.76

Explanation:

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