Question

1. A 0.17-mole sample of nitrogen gas occupies a volume of 2.80 L . What is the volume of 0.29 mol of nitrogen gas under the same conditions? Express your answer using two significant figures. V=

2. A sample of gas with an initial volume of 32.0 L at a pressure of 760 mmHg and a temperature of 320 K is compressed to a volume of 16.3 L and warmed to a temperature of 445 K . What is the final pressure of the gas? Pfinal =

3.

6. Use the combined gas law to complete the following table (assume the number of moles of gas to be constant): . Complete each column

P1	V1	T1	P2	V2	T2
1.16 atm	1.58 L	11.3 ∘C	1.64 atm	--	32.3 ∘C
718 torr	148 mL	126 K	803 torr	152 mL	--
5.59 atm	0.887 L	23.1 ∘C	--	1.03 L	39.2 ∘C

Answer 1

1. PV = nRT

V2/V1 = n2/n1

with,

V1 = 2.80 L

V2 = ?

n1 = 0.17 mole

n2 = 0.29 mole

we get,

V2 = 0.29 x 2.8/0.17 = 4.78 L

is the new volume

2. moles of gas = 1 atm x 32 L/0.08205 L.atm/K.mol x 320 = 1.22 mols

final pressure of gas = 1.22 x 0.08205 x 445/16.3 = 2.733 atm

3. Table will be completed using PV = nRT

Completed table

P1                    V1           T1            P2               V2             T2

1.16 atm       1.58 L      11.3 oC    1.64 atm      1.20 L       32.3 oC

718 torr        148 mL     126 K       803 torr     152 ml       144.72 K

5.59 atm       0.887 L     23.1 oC    5.07 atm    1.03 L        39.2 oC