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Questions and Answers
What is produced when dilute hydrochloric acid is added to iron fillings?
What is a balanced chemical equation?
What type of reaction produces water and sulfur dioxide from hydrogen sulfide gas?
What is produced when barium chloride reacts with aluminum sulfate?
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Which of the following is the balanced equation for the reaction of calcium hydroxide with carbon dioxide?
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Which type of reaction is identified by combining magnesium with hydrochloric acid to produce magnesium chloride and hydrogen?
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Why is respiration considered an exothermic reaction?
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Why are decomposition reactions called the opposite of combination reactions?
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What are the products of the reaction between barium chloride and potassium sulphate?
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Which type of reaction occurs when hydrogen gas burns in air?
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Which of the following signifies an exothermic reaction?
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What gas is produced when zinc reacts with hydrochloric acid?
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Which of the following reactions is a decomposition reaction?
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Which outcome is expected when calcium hydroxide reacts with carbon dioxide?
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Which of the following correctly identifies the products of the reaction between hydrogen and chlorine?
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What is the product when potassium reacts with water?
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Study Notes
Chemical Reactions and Equations
- When dilute hydrochloric acid is added to iron fillings, hydrogen gas and iron chloride are produced.
Balanced Chemical Equations
- A balanced chemical equation is an equation that has the same number of atoms of each element on both the reactant and product sides.
- Chemical equations should be balanced to ensure that the law of conservation of mass is upheld.
Chemical Equations and Reactions
- Hydrogen gas combines with nitrogen to form ammonia: N2 + 3H2 → 2NH3
- Hydrogen sulphide gas burns in air to give water and sulfur dioxide: 2H2S + 3O2 → 2H2O + 2SO2
- Barium chloride reacts with aluminum sulfate to give aluminum chloride and a precipitate of barium sulfate: 3BaCl2 + Al2(SO4)3 → 2AlCl3 + 3BaSO4
- Potassium metal reacts with water to give potassium hydroxide and hydrogen gas: 2K + 2H2O → 2KOH + H2
Balancing Chemical Equations
- HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O
- 2NaOH + H2SO4 → Na2SO4 + 2H2O
- NaCl + AgNO3 → AgCl + NaNO3
- BaCl2 + H2SO4 → BaSO4 + 2HCl
Chemical Reactions and Equations
- Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water: Ca(OH)2 + CO2 → CaCO3 + H2O
- Zinc + Silver nitrate → Zinc nitrate + Silver: Zn + 2AgNO3 → Zn(NO3)2 + 2Ag
- Aluminium + Copper chloride → Aluminium chloride + Copper: 2Al + 3CuCl2 → 2AlCl3 + 3Cu
- Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride: BaCl2 + K2SO4 → BaSO4 + 2KCl
Reaction Types
- Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + Barium bromide(s) (Precipitation reaction)
- Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g) (Decomposition reaction)
- Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g) (Combination reaction)
- Magnesium(s) + Hydrochloric acid(aq) → Magnesium chloride(aq) + Hydrogen(g) (Single displacement reaction)
Exothermic and Endothermic Reactions
- Exothermic reaction: A reaction that releases heat energy, e.g., combustion reactions.
- Endothermic reaction: A reaction that absorbs heat energy, e.g., decomposition reactions.
- Respiration is considered an exothermic reaction because it releases heat energy.
Combination and Decomposition Reactions
- Combination reaction: A reaction in which two or more substances combine to form a single product, e.g., 2H2 + O2 → 2H2O.
- Decomposition reaction: A reaction in which a single substance breaks down into two or more products, e.g., 2H2O → 2H2 + O2.
Chemical Reactions and Equations
- When dilute hydrochloric acid is added to iron fillings, hydrogen gas and iron chloride are produced.
Balanced Chemical Equations
- A balanced chemical equation is an equation that has the same number of atoms of each element on both the reactant and product sides.
- Chemical equations should be balanced to ensure that the law of conservation of mass is upheld.
Chemical Equations and Reactions
- Hydrogen gas combines with nitrogen to form ammonia: N2 + 3H2 → 2NH3
- Hydrogen sulphide gas burns in air to give water and sulfur dioxide: 2H2S + 3O2 → 2H2O + 2SO2
- Barium chloride reacts with aluminum sulfate to give aluminum chloride and a precipitate of barium sulfate: 3BaCl2 + Al2(SO4)3 → 2AlCl3 + 3BaSO4
- Potassium metal reacts with water to give potassium hydroxide and hydrogen gas: 2K + 2H2O → 2KOH + H2
Balancing Chemical Equations
- HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O
- 2NaOH + H2SO4 → Na2SO4 + 2H2O
- NaCl + AgNO3 → AgCl + NaNO3
- BaCl2 + H2SO4 → BaSO4 + 2HCl
Chemical Reactions and Equations
- Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water: Ca(OH)2 + CO2 → CaCO3 + H2O
- Zinc + Silver nitrate → Zinc nitrate + Silver: Zn + 2AgNO3 → Zn(NO3)2 + 2Ag
- Aluminium + Copper chloride → Aluminium chloride + Copper: 2Al + 3CuCl2 → 2AlCl3 + 3Cu
- Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride: BaCl2 + K2SO4 → BaSO4 + 2KCl
Reaction Types
- Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + Barium bromide(s) (Precipitation reaction)
- Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g) (Decomposition reaction)
- Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g) (Combination reaction)
- Magnesium(s) + Hydrochloric acid(aq) → Magnesium chloride(aq) + Hydrogen(g) (Single displacement reaction)
Exothermic and Endothermic Reactions
- Exothermic reaction: A reaction that releases heat energy, e.g., combustion reactions.
- Endothermic reaction: A reaction that absorbs heat energy, e.g., decomposition reactions.
- Respiration is considered an exothermic reaction because it releases heat energy.
Combination and Decomposition Reactions
- Combination reaction: A reaction in which two or more substances combine to form a single product, e.g., 2H2 + O2 → 2H2O.
- Decomposition reaction: A reaction in which a single substance breaks down into two or more products, e.g., 2H2O → 2H2 + O2.
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Description
Test your understanding of chemical reactions and equations with these multiple-choice questions. Learn how to balance chemical equations and why it's important.
