Have you found videos, websites, or explanations that helped you understand this chapter? Let us know and we'll add them to "Resources" part of this page for other students to use.

1 atm = 760 mmHg

1/ 760 = X/ 383

X= 0.5039

What is the pressure in torr of 1.47 atm?

760 torr = 1 atm

760 /1 = X / 1.47

X= 1117.2

What is the pressure in atm of a gas where n = 0.16 mol, V = 13.76 L, and T = 28.4^{o}C?

PV=nRT

28.4^{o}C= 301.55 K

R=0.08206

P(13.76) = (0.16)(0.08206)(301.55)

P=0.2877

What is the temperature in K of an ideal gas where P = 728 torr, n = 0.0271 mol, and V = 476.5 mL?

PV=nRT

(728/760)(.4765)=(0.0271)(0.08206)T

=205.24

How many moles of an ideal gas produce a pressure of 744 torr and a volume of 2.30 L at 285 K?

PV=nRT

(744/760)(2.30L) = n (0.08206)(285)

n=0.0962744

If the mass of the gas in the preceding problem is 33.1 g, what is the molar mass or molecular weight of the gas?

33.1 g / X MM = 0.0962744

X= 343.81

At a fixed temperature and number of moles of nitrogen gas, its volume and pressure are 196 mL and 687 torr, respectively. What is the final pressure in torr, if the final volume is 290 mL?

196(687)= 290 X

X=464.317

At a fixed pressure and number of moles, the initial volume and temperature of an air sample are 491 mL and 270 K, respectively. What is the final volume in mL, if the final temperature is 481 K?

V1/T1 = V2/T2

491/270 = X/481

874.707407

To what temperature in K must a variable volume container of helium gas be cooled to obtain a final volume of 0.255 L? The initial volume and temperature are 2.86 L and 332 K, respectively. The pressure and number of moles are fixed.

2.86/332 = 0.255 / X

X=29.601

A balloon filled with air and having no leak initially has a volume of 27.5 L, a pressure of 732 torr, and a temperature of 287 K. What is the final volume in L, if the final pressure is 489 torr and the final temperature is 244 K?

P1V1/T1 = P2V2/T2

(732)(27.5)/287 = (489)T/244

T=34.997

What is the total pressure if a container contains 59 torr of He gas, 234 torr of N_{2} gas, and 44 torr of Ar gas?

59 + 234 + 44 = 337

Oxygen gas is collected over water. The total pressure (the O_{2} pressure + the water vapor pressure) is 735 torr. The temperature of the water is such that the water vapor pressure is 44 torr. What is the partial pressure of the oxygen gas in torr?

735 - 44 = 691

What volume in L of chlorine at 30^{o}C and 702 torr is required to react completely with 4.48 g aluminum:

2Al(s) + 3Cl_{2}(g) → 2AlCl_{3}(s)

2Al(s) + 3Cl

Procedure: g Al --> mol Al --> mol Cl2. Next solve for V in PV = nRT. Did you remember to convert torr to atm and C to K?

4.48 g Al / 26.981 MM = 0.166 mol Al

0.166 mol Al * 3 mol Cl2/ 2 mol Al = 0.24906 mol Cl2

PV= nRT

(702/760)V= (0.24906)(0.08206)(303.15)

V = 6.54

**Question 15**

The pressure on a balloon holding 411 mL of an ideal gas is increased from 211 torr to 1.00 atm. What is the new volume of the balloon (in mL) at constant temperature?

(211torr) (411 mL) = (760torr) (V2)

V2 = (211 torr x 411 mL) / (760 torr) = 114 mL

**Question 16**

A sample of hydrogen gas (H2) is in a 2.07 L container at 531 torr and 24 C. Express the pressure of hydrogen in atm after the volume has changed to 1.30 L and the temperature is raised to 155 C.

V1 = 2.07 L

P1 = 531 torr --> 0.699 atm

T1 = 24C --> 297 K

V2 = 1.30 L

T2 = 155C --> 428 K

P2: { (2.07 L x 0.699 atm) x (428 K) } / {(297K) x (1.3 L) } = 1.60

**Question 17**

A sample of methane gas (CH4) at 29.1 C is either heated or cooled. The pressure increases from 1.52 atm to 3.61 atm, and the volume of the sample changes from 1.83 L to 4.04 L. To what temperature, in C, was the methane heated or cooled?

P1: 1.52 atm

V1: 1.83 L

T1: 29.1 --> 302.1 K

P2: 3.61 atm

V2: 4.04L

T2: (1.52 atm x 1.83 L) / (3.61 atm x 4.04L x 302.1 K) = 6.313E-4

T2: 1/ 6.313E-4 = 1583K - 273= 1310C