Gases
是非題
(1)
(2)
( ) 1.000 atm = 1.013 MPa
( ) At constant temperature and pressure, 1.0 L of Ar(g) contains about
twice the number of atoms as 1.0 L of Ne(g) because the molar mass of
Ar is about twice that of Ne.
( ) The conditions 0oC and 1 atm are called standard temperature and
pressure (abbreviated STP).
( ) For conditions of P, V, and T to be the same, the gases can be different
but the molar mass of gas in each container must be the same.
(3)
(4)
1
2
3
4
☓
☓
○
☓
5
6
7
8
9
10
11
12
13
14
15
16
選擇題
(1)
( )
(2)
( )
(3)
( )
(4)
(5)
( )
( )
(6)
( )
The molar volume of an ideal gas is (A) 0.08206 (B) 8.314 (C) 22.4 (D)
24.4 L at STP.
According to the kinetic molecular theory of gases, the average kinetic
energy of the gas particles is directly proportional to (A) the Kelvin
temperature (B) the molar mass (C) the pressure (D) the volume of the
gas.
Which statement is false? (A) 1 bar = 105 Pa (B) 1 torr = 1 mm Hg (C) 1
atm = 14.7 psi (D) 1 Pa = 1 N/cm2
1 atm = 1.013 x (A) 103 (B) 104 (C) 105 (D) 106 Pa
Which conditions of P and T are most ideal for a gas? (A) high P, high T
(B) high P, low T (C) low P, high T (D) low P, low T
What would happen to the average kinetic energy of the molecules of a
gas sample if the temperature of the sample increased from 20oC to
40oC? (A) It would be doubled (B) It would be halved. (C) No change
(D) None of these.
1
2
3
4
5
6
C
A
D
C
C
D
7
8
9
10
11
12
13
14
15
16
問答、計算題
(1)
An unknown gas has the volume of 14.3 mL at 22oC and 659 torr. Calculate the
volume at STP.
(2)
O2 is bubbled through water for collection and becomes saturated with water
vapor. The collected sample had a total pressure of 754 torr and a volume of
0.650 L. The vapor pressure of water is 21 torr at 22oC. (a) What is the partial
pressure of O2 gas? (b) How many moles of O2 gas are present?
(3)
N2(g) + 3H2(g) ⇄2NH3(g)
You add an equal number of moles of N2 and H2 in a balloon. The volume of
the balloon is 1.00 L before any reaction occurs. Determine the volume of the
balloon after the reaction is complete.
A sample of B2H6(g) has a pressure of 0.454 atm at -15oC and 3.48 L. If
conditions are changed so that the temperature is 36oC and the pressure is
0.616 atm, what will be the new volume of the sample?
Calculate the density of neon gas at 1.00 atm and 25.0oC. (1 Ne atom = 20.18
amu)
A 15.0 g sample of a hydrocarbon is placed in a balloon at 1.0 atm and 25oC
(4)
(5)
(6)
and the volume of the balloon is 12.2 L. The hydrocarbon is 79.89% carbon
and 20 11% hydrogen by mass. Determine the molecular formula of the
hydrocarbon.
(1)
11.5 mL
(2)
(a) 754 torr
(b) 2.59×10-2 mol
(3)
1.33 L
(4)
3.07 L
(5)
0.825 g/L
(6)
C2H6