If I have 0.275 moles of gas at a temperature of 75 K and a pressure of 17.5 psi, what is the volume of the gas?

V = 1.4 L

General Formulas and Concepts:

Chem

Ideal Gas Law: PV = nRTConstant R = 0.8206 L · atm/mol14.7 psi = 1 atmIdeal Gas Law:

Explanation:

Step 1: Define variables

n = 0.275 moles

T = 75 K

P = 17.5 psi

V = unknown

Step 2: Solve for V

Convert psi to atm:          17.5 psi = 1.19048 atmSubstitute:                        1.19048 atm · V = (0.275 mol)(0.08206)(75 K)Multiply:                            1.19048V = 1.69249Isolate V:                           V = 1.42169 L

Step 3: Check

Our smallest sig figs is 2. Follow sig fig rules.

1.42169 L ≈ 1.4 L

The answer is 1.42 L

Explanation:

In order to find out the volume of the gas we use the Ideal Gas Equation

PV = nRT

where

P is the pressure

V is the volume of the gas

n is the number of moles

R is the gas constant which is

8.314 JK-¹mol-¹ or 0.0821 dm³ atm.mol-1K-¹

T is the temperature in Kelvin

Since we will be converting the pressure to atm , for the gas constant we use

0.0821 dm³ atm.mol-1K-¹

From the question

17.5 psi = 1.19 atm

Since we are finding the volume , we make V the subject

We have

n = 0.275 moles

T = 75 K

We have

We have the final answer as

1.42 L

Hope this helps you

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Ais the correct answer