Chem Gas Worksheet 3. Block:
Teacher: ________
100KPa=750.1mmHg=0.987atm=14.5lb/sq.in.
One-variable Ideal Gas Laws. SHOW SET-up.
Name: _________________________
24.8L/mol @ SATP (298.15K, 100kPa.)
Boyle's Law: P vs. V, n & T constant.
a. 75L of a gas at 27atm. will occupy what volume at 30.atm?
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b. 389 cm3 of gas at 178kPa will occupy 652 cm3 at what pressure?
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c. To what pressure must 2.222L of gas, measured at 910.6mmHg, be raised to reduce its
volume to 765.5cm3?
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Gay-Lussac's Law: P vs. T, V & n constant. MUST USE ABSOLUTE
TEMPERATURES!
d. At 250.K a gas had a pressure of 0.853atm. At what temperature would it be at 1.32atm?
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e. A gas at 375K produced a pressure of 135kPa. What pressure would it have at 225K?
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f. At -39°C a gas was at 469mmHg. At what temperature would it reach 1.00atm?
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Charles' Law: V vs. T, P & n constant. ABSOLUTE TEMPERATURES ONLY.
g. A gas occupied 729mL at 228K. What volume would it have at 337K?
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h. A gas at 167.5K measured 1.111L. At what temperature would it occupy 2.505L?
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i. 134.5 mL of a gas at -125.3°C. At what temperature would it occupy 1.000L?
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Avogadro's Law: V vs. n, P & T constant.
j. 2.0 moles filled up 32 liters. What number of moles would occupy 8.8L at the same temp.
and pressure?
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k. 752 cm3 contained 0.0438 moles. What volume would hold 1.65 moles?
l. At SATP, how many moles are needed to occupy 1750 cm3?
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m. A container held 0.0750 moles of O2. The same container at the same temperature
and pressure held 9.00 g of gas "Q". What was the molecular mass of gas "Q"?
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n. At an unknown temperature and an unknown pressure, a flask of unknown volume holds
2.016g of oxygen gas. At the same temperature and pressure the same flask holds 8.245 g
of gas "X" What is the molecular weight of gas "X"?
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Dalton's Law: P vs. n, V & T constant.
o. 0.225 moles produced 155kPa. What pressure would result from 0.552 moles.
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p. 2.375 moles of gas produced 1192mmHg. How many moles would it take to get 1.000atm?
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q. 0.350 moles of Ne produced 124 kPa. 0.142 moles of Ar were added. What was the total
pressure?
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r. How many moles of Kr must be added to a container with 0.08733 mol O2 to raise the
pressure from 131.2kPa to 200.0kPa?
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s. 0.3333 mol of gas in a container produced 50.0kPa. 1.00 g H2, 2.00 g N2, 4.00 g Ar, and
6.00 g CO2 were added. What was the partial pressure of each gas, and the total pressure in the
container?
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"Unnamed" Law: n vs. T, P & V constant.
t. 3.0 moles of gas were at 400.K. How many moles would be needed to produce the same
pressure at 250K?
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u. 0.4672 mol at 295.5K. What temperature would be needed to produce the same pressure
with 0.1989mol?
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v. 0.575 mol produced 1.00atm. at -30.°C. How many moles of gas must be released from
the container in order to keep the pressure the same when the temperature is increased to
65°C?
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