Gases 1.If a gas sample at constant temperature has a volume of 21.3 Ml at 764 t

Question

Gases

1.If a gas sample at constant temperature has a volume of 21.3 Ml at 764 torr, what will the volume be at 546 torr?

2. A 5.40 L gas sample at 854 torr is compressed at 1.35atm to what volume?

3. At constant pressure, a gas sample occuies 379 ml at 23 degrees celcius. At what temperature will the volume be doubled?

4. What will be the volume of a gas sample containing 12.4 grams of carbon dioxide at STP?

5. If a gas at 25 degrees celcius and 755 torr has a volume of 333 ml, what would its volume be at STP?

6. How many grams of chlorine are contained in 57.5ml of gas at 26 degrees celcius and 786 torr?

7. What pressure, in torrs, will be exerted by 3.57 grams of nitrogen monoxide at 34 degrees celcius if its volume is 59.0ml?

8. What is the molar mass of a gas if 286ml at 69 degrees celcius and 17.9 torr pressure weighs 0.0156?

9. What is the molar mass of a gas if its density at 16 degrees celcius and 0.980 atm is found to be 2.66 g/L?

10. Calculate the density of a gas if at 30 degrees celcius it has a pressure of 0.398 atm. Molar mass of the gas is 80g/mole?

Explanation / Answer

1.If a gas sample at constant temperature has a volume of 21.3 Ml at 764 torr, what will the volume be at 546 torr?

P1V1 = P2V2

21.3 X 764 = v2 X 546

V2 = 298.mL

2. A 5.40 L gas sample at 854 torr is compressed at 1.35atm to what volume?

P1V1 = P2V2

1.35 atm = 1026 torr

5.4X 854 = 1026 X V2

V2 = 4.49L

3. At constant pressure, a gas sample occuies 379 ml at 23 degrees celcius. At what temperature will the volume be doubled?

V1 / T1 = V2 / T2

379 / 296 = 2 X 379 / T2

T2 = 2 X 296 = 592 K

4. What will be the volume of a gas sample containing 12.4 grams of carbon dioxide at STP?

PV = nRT

n=moles = mass / mol wt = 12.4 / 44 = 0.2818

P = 1atm

T = 273 K

R = 0.0821

V = 0.2818 X 0.0821 X 273 / 1 = 6.831L

5. If a gas at 25 degrees celcius and 755 torr has a volume of 333 ml, what would its volume be at STP?

P1V1/ T1 = P2V2/ T2

755 X 333 / 298 = Volume X 760 / 273

Volume = 303.05mL

6. How many grams of chlorine are contained in 57.5ml of gas at 26 degrees celcius and 786 torr?

PV=nRT

P = 786 torr = 1.03 atm

V = 57.5 mL = 0.057 L

T = 299 K

n = 1.03 X 0.057 / 299 X 0.0821 = 0.0023 moles

mass = moles X mol wt = 0.0023 X 71 =0.169g

7. What pressure, in torrs, will be exerted by 3.57 grams of nitrogen monoxide at 34 degrees celcius if its volume is 59.0ml?

PV = nRT

n = mass / mol wt = 3.57 / 28 = 0.1275 moles

P = 0.1275 X 0.0821 X 307 / 0.059L = 54.4 atm = 41344 torr

8. What is the molar mass of a gas if 286ml at 69 degrees celcius and 17.9 torr pressure weighs 0.0156?

P = 17.9 torr = 0.023 atm

V = 0.286 L

T = 342 K

N = ?

PV = nRT

n = PV / RT

n = 0.023 X 0.286 / 0.0821 X 342 = 2.3 X 10^-4

molar mass = mass / moles = 0.0156 / 2.3 X 10^-4 = 67 g

9. What is the molar mass of a gas if its density at 16 degrees celcius and 0.980 atm is found to be 2.66 g/L?

PV = nRT

PV = mass R T / mol wt

Or mol wt = mass X R X T / PV

Mol wt = density XR X T / P =2.66 X 0.0821 X 289 / 0.98 = 64.4 g

10. Calculate the density of a gas if at 30 degrees celcius it has a pressure of 0.398 atm. Molar mass of the gas is 80g/mole?

Density = mol wt X P / RT = 80 X 0.398 / 0.0821 X 303 = 1.279 g /L

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