An 8.50 L tire contains 0.552 mol of gas at a temperature of 305 K. What is the pressure (in atm and in psi) of the gas in the tire? (1 atm is approximately equal to 14.7 psi.) Express the pressures in atmospheres and pounds per square inch to three significant figures separated by a comma.

1. The pressure of the gas in atm is 1.63 atm.

2. The pressure of the gas in psi is 24 psi.

1. Determination of the pressure in atm.

Volume (V) = 8.50 L

Number of mole (n) = 0.552 mole

Temperature (T) = 305 K

Gas constant (R) = 0.0821 atm.L/Kmol

P × 8.5 = 0.552 × 0.0821 × 305

P × 8.5 = 13.822356

Divide both side by 8.5

P = 13.822356 / 8.5

Thus, the pressure of the gas in atm is 1.63 atm

2. Determination of the pressure of the gas in psi

Pressure (in atm) = 1.63 atm

1 atm = 14.7 psi

Therefore,

1.63 atm = 1.63 × 14.7

1.63 atm = 23.961 psi

Thus, the pressure of the gas in psi is 24 psi.

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pressure = 1.625 atm or 23.89 psi

Explanation:

Step 1: Data given

Volume = 8.50 L

Number of moles of gas

Temperature = 305 K

Step 2: Calculate pressure

p*V = n*R*T

⇒with p = the pressure of the gas = TO BE DETERMINED

⇒with V= the volume of the gas = 8.50 L

⇒with n = the number of moles of gas = 0.552 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 305 K

p = (n*R*T)/V

p = (0.552*0.08206*305)/8.50

p = 1.625 atm

1.625 * 14.7 = 23.89

1.625 atm = 23.89 psi

-be a crystalline solid

- be soluble in water

-conduct electricity

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