Unit 4: Chemical Reactions

Which describes an oxidation-reduction reaction?

If 5.00 g of NaCl (molar mass 58.44 g/mol) are dissolved in water to make 250.0 mL of solution, what is the molarity? Round to 3 decimal places.

When the equation _Fe + _O₂ → _Fe₂O₃ is balanced, the coefficients are

In a reaction between 10.0 g of hydrogen gas (H₂) and 10.0 g of oxygen gas (O₂), the limiting reactant is

A 0.500 g sample of an unknown metal reacts with excess hydrochloric acid to produce 224 mL of H₂ gas at STP. Given the equation M + 2HCl → MCl₂ + H₂, the molar mass of the metal is approximately

In the net ionic equation for the reaction between aqueous sodium hydroxide and aqueous hydrochloric acid, the spectator ions are

Which of the following is an oxidation-reduction (redox) reaction?

A student performs a gravimetric analysis by adding excess BaCl₂ to 50.0 mL of a Na₂SO₄ solution. The resulting BaSO₄ precipitate, after filtering and drying, has a mass of 1.165 g. The concentration of Na₂SO₄ in the original solution is

In the reaction 2KMnO₄ + 16HCl → 2KCl + 2MnCl₂ + 5Cl₂ + 8H₂O, the oxidation state of Mn changes from

What volume of 0.250 M HCl is needed to neutralize 25.0 mL of 0.100 M NaOH?

In the reaction Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g), the substance being oxidized is

A net ionic equation shows:

In a redox reaction, the substance that is oxidized:

The mole concept is useful because it:

The limiting reagent in a reaction is:

Stoichiometry uses mole ratios from balanced equations to:

Gravimetric analysis determines the amount of a substance by:

Spectrophotometry uses Beer's Law to relate:

Percent yield is calculated as:

If 5.00 g of iron reacts with excess O₂, what mass of Fe₂O₃ is produced?

Which reagent is the limiting reagent and how many moles of water are produced?

What is the percent yield of this reaction?

What is the net ionic equation for the reaction between these two solutions?

What is the oxidation state of manganese in KMnO₄?

Which reaction is an example of a redox reaction?

What is the mass percent of chloride in the original sample?

What volume of NaOH (in mL) is needed to completely neutralize the HCl solution?

A student adds excess zinc metal to 100.0 mL of 0.500 M CuSO₄ solution. After the reaction is complete, which of the following observations would the student most likely make?

When 0.50 mol of propane (C₃H₈) undergoes complete combustion, how many moles of CO₂ are produced? C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

In the reaction: 2 KMnO₄ + 16 HCl → 2 KCl + 2 MnCl₂ + 5 Cl₂ + 8 H₂O, the oxidation state of Mn changes from

In a titration, 35.0 mL of 0.150 M NaOH is required to completely neutralize 25.0 mL of an unknown HCl solution. What is the molarity of HCl?