Chemistry Practice Test 13 - 14
What do the initials STP stand for, and what are the numerical values of each?
- standard temperature = 273K - pressure = 1 atm
The specific heat capacity of liquid water is 4.18 J/g°C. Calculate the quantity of energy required to heat 10.0 g of water from 26.5°C to 83.7°C.
2.39 x 10³ (Swater)
263kPa = _________ Pa
2.63 x 10⁵ (263*1000)
One mole of CO2 at STP will occupy
22.4 L
What volume will 28.0 g of N2 occupy at STP?
22.4 L
What is the numerical value of the molar volume of any gas at STP?
22.4 L/mol
1L - ml
1000 ml
1 kpa - pa
1000 pa
1 atm - pa
101,325 pa
A sample of helium gas occupies 2.65 L at 1.20 atm. What pressure would this sample of gas exert in a 1.50 L container at the same temperature?
2.12 atm (P1V1=P2V2)
1 kpa - mm hg
7.500617 mm hg
1atm - mm hg - torr
760 mm hg - and - 760 torr
The Pvap for water at 100.0°C is
760 torr
1.13 atm = ________ torr
859 (1.13*760)
KBr
ionic
Which conditions of P and T are most ideal for a gas?
low P, high T
At 1 atmosphere of pressure, liquid water always changes to gaseous water at 100°C.
true
An ideal gas is a hypothetical substance consisting of particles with _____ volume and _____ attraction for one another.
zero; no
H₂O
Hydrogen bond
The intermolecular forces called hydrogen bonding will not exist between molecules of
H₂
highest boiling point : H₂, O₂, H₂O
H₂
more volatile : H₂O or H₂S
H₂S
highest boiling point : Ga, KBr, O₂
KBr
CH₄
LDF
CO₂
LDF
Kr
LDF
N₂
LDF
As the atmospheric pressure around a liquid decreases, the boiling temperature of the liquid
decreases
Identify the major attractive force in each of the following molecules - H₂S
dipole-dipole
NF₃
dipole-dipole
If temperature and pressure are held constant, the volume and number of moles of a gas are
directly proportional
CH₃OH
hydrogen bond
A sample of a gas at 0.75 atm occupies a volume of 521 mL. If the temperature remains constant, what will be the new pressure if the volume increases to 776 mL?
0.50atm (P1V1=P2V2)
A 6.5 L sample of nitrogen at 25°C and 1.5 atm is allowed to expand to 13.0 L. The temperature remains constant. What is the final pressure?
0.75 atm (P1V1=P2V2)
An 11.7-L sample of gas is determined to contain 0.60 mol of nitrogen gas. At the same temperature and pressure, how many moles of gas would there be in a 25.0-L sample?
1.3 mol (N1/V1=N2/V2)
A sample of helium gas occupies 12.4 L at 23°C and 0.956 atm. What volume will it occupy at 40°C and 0.956 atm?
13.1 L (P1V1/T1=P2V2/T2)
1atm - psi
14.7 psi
Calculate the quantity of energy required to change 26.5 g of liquid water to steam at 100°C. The molar heat of vaporization of water is 40.6 kJ/mol.
59.8 kJ (26.5/18*40.6)
more volatile : CH₃CH₃ or CH₃CH₂CH₃
CH₃CH₃
more volatile : H₂O or CH₃OH
CH₃OH
Which compound is more likely to be a gas at room temperature (as opposed to a liquid)?
C₂H₆
highest boiling point : Hg, NaCl, He
NaCl
Which of the following is most likely to be a solid at room temperature?
Na₂S
Which of the following statements is true about the kinetic molecular theory?
Pressure is due to the collisions of the gas particles with the walls of the container.
Name the type of crystalline solid formed by copper.
atomic solid