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WorksheetsGeneral Chemistry Review Game
Total questions: 23
Worksheet time: 6hrs 45mins
What is Boyles Law?
P1V1=P2V2
V1/T1=V2/T2
T1/V1=T2/V2
P1T1=P2T2
What happens to a balloon volume when the temperature increases? What gas law is that?
Decrease, Boyle Law
Increase, Boyle Law
Decrease, Amontons Law
Increase, Amontons Law
Stays the same
A balloon is filled with 35.0 L of helium in the morning when the temperature is 20.00 C. By noon the temperature has risen to 45.00 C. What is the new volume of the balloon?
38.0mL
38.0L
32.35mL
32.35L
A helium balloon with an internal pressure of 1.00 atm and a volume of 4.50 L at 20.00 C is released. What volume will the balloon occupy at an altitude where the pressure is 0.600 atm and the temperature is –20.00 C?
6.48L
0.16L
3.23L
10.14L
What is Dalton's Law?
law states that the rate of diffusion or of effusion of a gas is inversely proportional to the square root of its molecular weight
law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases
law states that the total pressure exerted is equal to the partial pressures of each individual part of a solution
law states that the total rate of diffusion or effusion of a gas is directly proportional to the square root of its molecular weight
A 2.00 L mixture of helium, nitrogen, and neon has a total pressure of 815 mmHg at a room temperature of 255K. If the partial pressure of helium is 201 mmHg and the partial pressure of nitrogen is 351 mmgHg, what is the partial pressure of neon?
(a)
A compound composed of carbon, hydrogen, and chlorine diffuses through a pinhole 0.411 times as fast as neon. Select the correct molecular formula for the compound:
Hint: Use Graham's Law
CHCl3
~119g
CH2Cl2
~85g
C2H2Cl2
~97g
C2H3Cl
~64g
Based on the partial pressure of Nitrogen from the last question, what is the mass of Nitrogen that is present.
0.601 g
0.667 g
0.709 g
0.512 g
Which substance would have the weakest intermolecular forces of attraction
CH4
NaCl
H2O
MgF2
Between 1-butanol, 2-butanol, and butane....who would have the highest vapor pressure?
1-butanol
2-butanol
butane
Put these in INCREASING boiling point temperature
HCl H2O SiH4
HCl<SiH4<H2O
H2O<HCl<SiH4
H2O<SiH4<HCl
SiH4<HCl<H20
The boiling points of the halogens increase in order of F2<Cl2<Br2<I2 due to the increasing (a) interaction?
Which one has the highest melting point?
BaF2
BaCl2
BaBr2
BaI2
NaF
All of the following statements, except one, are important postulates of the kinetic-molecular theory of gases. Which one?
Gases consist of large numbers of particles in rapid random motion.
The volume of the molecules of a gas is very small compared to the total volume in which the gas is contained.
The average kinetic energy of the molecules is inversely proportional to the absolute temperature.
The time during which a collision between two molecules occurs is negligibly short compared to the time between collisions.
There are no attractive or repulsive forces between the individual molecules.
Use the Root-mean-square velocity for a nitrogen molecule at 25°C
R=8.314 J/molK
(a)
Where is liquid phase located?
A
B
C
Where is the gas phase located?
A
B
C
What is the name of the phase change that occurs when a solid turns into a gas?
evaporation
melting
sublimation
deposition
At -95C and 11atm what phase would water be in?
solid
liquid
gas
vapor
Where does melting occur?
A -> B
C -> D
D->C
B -> C
B -> A
What is happening to water from E -> D?
liquid water is boiling
liquid water is heating up
steam is condensing
steam is losing heat
What is the equation needed to determine how much heat is needed to melt the ice
q=mct
q=mΔHfusion
q=mΔHvaporization
How much heat is required to convert 135g of ice at -15C into water vapor at 120 C
(a)
