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Gas Law
Dilutions/Tirations
R A N D O M
Partial Pressure
Redox rxns, oxidation states, or other things
100
If I have 4.00 moles of a gas at a pressure of 5.60 atm and a volume of 12.0 liters, what is the temperature?
205 K
100
If 45 mL of water are added to 250 mL of a 0.75 M K2SO4 solution, what will the molarity of the diluted solution be?
0.64 M
100
Balance this equation: 

Na3PO4(aq) + AgNO3(aq) → NaNO3(aq) + Ag3PO4(s)

1, 3, 3, 1
100
A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?
9.00 atm
100
What is the oxidation state of Nitrogen in N2O4
+4
200

A cylinder contains 28.5 L of oxygen gas at a pressure of 1.8 atm and a temperature of 298 K. How much gas (in grams) is in the cylinder? (R = 0.08206)

76 grams

200
Calculate the volume of 0.500 M NaCl needed to prepare 200 mL of a 0.150 M NaCl solution.
60 mL
200
What is the formula for Lead (II) sulfite?
PbSO3
200
If 60.0 L of nitrogen is collected over water at 40.0 °C when the atmospheric pressure is 760.0 mmHg, what is the partial pressure of the nitrogen in atm? (pressure of water at 40°C is 55.3 mmHg) (760 mmHg = 1 atm)
0.927 atm
200
Identify the species being reduced in the following reaction: 3 Hg2+ + 2 Fe (s) --> 3 Hg2 + 2 Fe3+
Hg2+
300

What is the density of of N2 gas at a pressure of 1.8 atm at 300 K?

2.05 g/L

300
You have performed a titration on a 30.00 mL sample of HCl. To reach the endpoint of the titration, you added 40.78 mL of 0.130 M NaOH. How many moles of NaOH did you add?
5.30 X 10^-3 moles NaOH
300
After completing the reaction, write the net ionic equation. KI (aq) + Pb(NO3)2(aq) -->
Pb2+ (aq) + I-(aq) --> PbI2 (s)
300
A tank contains 5.00 moles of O2, 3.00 moles of neon, 6.00 moles of H2S, and 4.00 moles of argon at a total pressure of 1620.0 mmHg. What is the partial pressure of H2S in the tank?
540. mmHg or 0.711 atm
300
Would you use a oxidizing or reducing agent in order for this reaction to occur? Zn --> ZnCl2
oxidizing agent
400

A gas is heated from 263.0 K to 298.0 K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be?

0.777 atm

400
Calculate the number of mL of 2.00 M HNO3 solution required to react with 216 grams of Ag according to the equation: 

3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) 

(molar mass of Ag is 107.87 g/mol)

1.33 X 10^3 mL HNO3
400
Name or write the proper formula for these acids (must get each part correct to receive credit): (a) HNO3 (b) carbonic acid (c) H2S
(a) nitric acid (b) HCO3 (c) Hydrosulfuric acid
400
The oxygen gas emitted by an aquatic plant is collected over water at a temperature of 293K and a total pressure of 855.2 mmHg. A total of 2.50 L of gas is collected. What mass of oxygen gas is formed? (760 mmHg = 1 atm) (at 293 K, the pressure of water is 17.55 mmHg)
3.67 grams O2
500
A titration was performed based on the following equation: 

 H2C2O4 (aq) + KOH (aq) → K2C2O4 (aq) + H2O (l)

In this titration, 44.55 mL of KOH was added to neutralize 15.00 mL of 0.0800 M H2C2O4. What was the concentration (in M) of KOH in the sample?

0.0538 M KOH
500
Consider the unbalanced reaction: 

Al + HBr → AlBr3 + H2 

When 3.22 moles of Al reacts with 4.96 moles of HBr, how many grams of H2 are formed?

5.01 grams
500
A tank contains 480.0 grams of oxygen and 80.00 grams of helium at a total pressure of 7.00 atmospheres. Calculate (a) the mole fraction of He and (b) the partial pressure of O2. Must complete both parts to get credit for question
(a) 0.5714 (b) 3.00