Ch 7
Ch 8
Ch 9
100

What happens during an exothermic reaction? Draw an example of the diagram.

The chemical reaction releases energy

100

According to the kinetic molecular theory, how does the temperature of a gas affect the speed of its particles?

The kinetic molecular theory states that the average kinetic energy of gas particles is directly proportional to the temperature of the gas in kelvins. As the temperature increases, the kinetic energy of the particles also increases, causing the particles to move faster. Conversely, at lower temperatures, the particles move more slowly.

100

If sodium bicarbonate (NaHCO3) dissolves in water, what ions will form in solution?

Na+ and HCO3-

200

  1. How many molecules are present in 0.500 moles of glucose (C₆H₁₂O₆)?

  2. How many atoms of hydrogen (H) are in 0.500 moles of glucose?

3.011 x1023 molecules

3.61 x1024 atoms H

200

A 3.0 L sample of a gas is kept at 300 K under 1.5 atm of pressure and consists of 0.25 moles. What will the volume of this gas be if the temperature is increased to 600 K and the pressure is raised to 4.0 atm?

2.25 L

200

At 50 °C, the solubility of KNO₃ is 150 g per 100 g of water. If 180 g of KNO₃ is added to 120 g of water at 50 °C, is this solution saturated or unsaturated?

Saturated 

300

What mass of CO is needed to completely react with 0.500 moles of Fe₂O₃ (s) based on the reaction below?

Fe₂O₃ (s) + 3CO (g) → 2Fe (s) + 3CO₂ (g)

42.02 grams of CO

300

A sample of ammonia gas (NH3) has a pressure of 850 mmHg and occupies a volume of 250 mL at a temperature of 310 K. How many moles of ammonia gas are present in the sample?

0.0110 moles

300

What is the mass percent (m/m) of NaOH in a solution prepared by dissolving 40.0 g of NaOH in 60.0 g of water?

40%

400

If 5.00 g of C2H4 (ethylene) and 12.00 g of O2 are the initial reactants, how many moles of carbon dioxide can be produced, and what is the limiting reactant?

The balanced equation for the reaction is:

C2H4+3O2→2CO2+2H2O

  • Limiting reactant: O2
  • Moles of CO2 produced: 0.250 mol
400

A gas mixture contains 5.0% hydrogen (H2), 70.0% oxygen (O2), and 25.0% nitrogen (N2) by volume. The total pressure of the mixture is 1.8 atm.

What is the partial pressure of each gas in the mixture?

  • H2: 0.090 atm
  • O2: 1.26 atm
  • N2: 0.450 atm
400

Predict whether the following compounds will be soluble in water:

  1. Ba(OH)2 

  1. ZnCl2

  1. AlPO4

  1. AgBr

  1. Ba(OH)2 - soluble

  1. ZnCl2 - soluble

  1. AlPO4 - insoluble 

  1. AgBr - insoluble

500

A chemist is performing the reaction between nitrogen gas and hydrogen gas to produce ammonia. They start with 10.0 g of N2 and 5.0 g of H2. The balanced chemical equation for the reaction is:

N2+3H2→2NH3

  1. Determine the limiting reactant and the theoretical yield of ammonia.
  2. If the reaction yields 12.5 g of ammonia, calculate the percent yield.
  • Limiting reactant: N2
  • Theoretical yield: 12.15 g of NH3
  • Percent yield: 102.9%
500

Under standard conditions, a chemist collects 44.8 liters of carbon dioxide gas (CO2) produced from the reaction of calcium carbonate (CaCO3) with hydrochloric acid (HCl) according to the reaction:

CaCO3+2 HCl→CaCl2+CO2+H2O 

  1. How many moles of CO2 gas are produced at STP?

  2. If the chemist started with 5.0 moles of HCl, which reactant is the limiting reactant?

  • Moles of CO2 produced: 2.00 mol
  • Limiting reactant: CaCO3
500

When solutions of barium chloride (BaCl₂) and sodium sulfate (Na₂SO₄) are mixed, a reaction occurs. Determine the precipitate formed, and write both the complete ionic equation and the net ionic equation.

  • Precipitate formed: BaSO4
  • Complete Ionic Equation: Ba2+(aq)+2Cl−(aq)+2Na+(aq)+SO42−(aq)→BaSO4(s)+2Na+(aq)+2Cl−(aq)
  • Net Ionic Equation: Ba2+(aq)+SO42−(aq)→BaSO4(s)
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