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What is the mass of a 8156.2 mL sample of hydrogen gas at 99.7oC and 69.49 kPa

What is the mass of 2.04 L of ammonia gas at STP?

What is the molar volume for a gas at -118.2oC and 2168.28 mmHg?

What is the density of sulfur dioxide gas at STP?

Feb 7th, 2015

Please note that, I apply the equation of gases, as below:

P*V=n*R*T, where n is the number of mol of the gas, V is the volume occupied by the gas, P is the pressure exerted by the gas, R is the constant of the gases, namely R = 0.08206 liter*atm/ °K. So we have:

Question 1)

n = (P*V)/(R*T) = (0.68 * 8.1562) /( 0.08206*372.85) = 0.18 mol of H2 gas

then the mass of H2 is 0.18* 2 = 0.36 grams

Please note thatthe pressure is 69490/101325 = 0.68 atm

and the temperature is:

273.15+99.7= 372.85 °K

Question 2)

here we have molecular mass of ammonia (NH3) = 17,

so n= (P*V) / (R*T)= (1*2.04)/(0.08206*273.15) = 0.091 mol of NH3,

so the mass of ammonia is 0.091 * 17 = 1.55 grams of NH3 gas.

Please note that the STP condition are T = 273.15 °K and P = 1 atm.

Question 3)

here we can write:

V/n = R*T/P = 0.08206*154.95 / 2.853 = 4.46 liter/mol,

since the temperature is T = 273.15-118.2= 154.95, and the pressure P is 2168.28/760 = 2.853 atm.

Question 4)

here we have molecular mass of SO2 = 64,

density = (P* molecular mass) / (R*T) = (1*64)/(0.08206*273.15) = 2.855 grams/liter

Feb 7th, 2015

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Feb 7th, 2015
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Feb 7th, 2015
Sep 23rd, 2017
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