Ch. 10
Given: 2 AgNO3 + BaCl2 --> 2 AgCl + Ba(NO3)2
If 410.8 grams of barium nitrate are produced how many grams of silver nitrate were reacted?
534.1 g AgNO3
If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume?
23.2 L
If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?
204.63 K
Identify the strongest intermolecular force present in pure samples of the following substance: SO2
Dipole-dipole
Define solution.
Homogeneous mixture of two or more substances in a single physical state
Given: N2(g) + 3 H2(g) --> 2 NH3(g)
How many liters of nitrogen trihydride are produced at STP if 80.28 grams of hydrogen gas are reacted in an excess of nitrogen?
594.7 L NH3
A container containing 5.00 L of a gas is collected at 100 K and then allowed to expand to 20.0 L. What must the new temperature be in order to maintain the same pressure (as required by Charles' Law)?
400 K
If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 0 C, how many moles of gas do I have?
1.2586 mol
Identify the strongest intermolecular force present in pure samples of the following substance: H2O
Hydrogen bonds
Calculate the molar concentration (Molarity, M) of each of the following solution: 2.3 moles of sodium chloride in 0.45 liters of solution
5.1 M
Given: N2(g) + 3 H2(g) --> 2 NH3(g)
How many grams of hydrogen are needed to fully react 621.9 grams of nitrogen gas?
134.3 g H2
The gases in a hair spray can are at a temperature of 27o C and a pressure of 30 lbs/in2 . If the gases in the can reach a pressure of 90 lbs/in2 , the can will explode. To what temperature must the gases be raised in order for the can to explode? Assume constant volume. (630 o C)
900 K
If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container?
1.642 atm
Identify the strongest IMF present in HF. Explain how you determined your answer.
Hydrogen Bonding
Molecules that have hydrogen attached to an O, N, or F can form hydrogen bonds. These are the strongest of the intermolecular forces.
Calculate the molar concentration (Molarity, M) of each of the following solution: 1.2 moles of calcium carbonate in 1.22 liters of solution
0.98 M
Given: N2(g) + 3 H2(g) --> 2 NH3(g)
How many liters of nitrogen gas are needed to completely react 90.38 L of hydrogen gas at STP?
30.09 L N2
If 10.0 liters of oxygen at STP are heated to 512 °C, what will be the new volume of gas if the pressure is also increased to 1520.0 mm of mercury?
13.2 L
If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0 C, what is the volume of the container that the gas is in?
2310.93 K
What are the three main IMFs? Describe them.
London Dispersion - The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.
Dipole-Dipole - Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
Hydrogen Bonding - A hydrogen bond is an intermolecular force (IMF) that forms a special type of dipole-dipole attraction when a hydrogen atom bonded to a strongly electronegative atom exists in the vicinity of another electronegative atom with a lone pair of electrons
Calculate the molar concentration (Molarity, M) of each of the following solution: 0.75 moles of lithium fluoride in 65 mL of solution.
11.5 M