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3.1 Introducing chemical reactions

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Question 10
F

A student adds silver nitrate solution to sodium iodide solution. A yellow precipitate of silver iodide forms. Sodium nitrate is soluble in water.

Which equation has the correct state symbols?

[1]
A

AgNO3(aq)+NaI(aq)→AgI(aq)+NaNO3(s)\mathrm{AgNO_{3}(aq) + NaI(aq) \rightarrow AgI(aq) + NaNO_{3}(s)}AgNO3​(aq)+NaI(aq)→AgI(aq)+NaNO3​(s)

B

AgNO3(aq)+NaI(aq)→AgI(s)+NaNO3(aq)\mathrm{AgNO_{3}(aq) + NaI(aq) \rightarrow AgI(s) + NaNO_{3}(aq)}AgNO3​(aq)+NaI(aq)→AgI(s)+NaNO3​(aq)

C

AgNO3(aq)+NaI(aq)→AgI(s)+NaNO3(l)\mathrm{AgNO_{3}(aq) + NaI(aq) \rightarrow AgI(s) + NaNO_{3}(l)}AgNO3​(aq)+NaI(aq)→AgI(s)+NaNO3​(l)

D

AgNO3(l)+NaI(l)→AgI(s)+NaNO3(l)\mathrm{AgNO_{3}(l) + NaI(l) \rightarrow AgI(s) + NaNO_{3}(l)}AgNO3​(l)+NaI(l)→AgI(s)+NaNO3​(l)

Markscheme

3.1 Introducing chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /3.1 Introducing chemical reactions

55 exam-style questions on OCR GCSE Chemistry 3.1 Introducing chemical reactions, covering 3.1.1 Writing formulae and balanced chemical equations, 3.1.2 Formulae of compounds from ions, and state symbols, 3.1.3 Conservation of mass and observed changes in mass, 3.1.4 Half equations and balanced ionic equations, 3.1.5 The mole and the Avogadro constant, and 3.1.6 Stoichiometry, limiting reactants and reacting masses. Each one has a worked solution and a mark scheme showing where the marks go.

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