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3 years ago

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:

(P₁V₁) = (P₂V₂)

Knowing that:

P₁ = 894.0 torr, V₁ = 534.0 mL,

P₂ = ??? torr, V₂ = 167.0 mL.

Applying in the above equation

(P₁V₁) = (P₂V₂)

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

To convert from torr to atm:

1.0 atm = 760.0 torr.

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

daser333 [38]3 years ago

8 0

Answer:

B)3.76

Explanation:

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