$$\(71.0 \mathrm{~g}\)$$ of chlorine, $$\(\mathrm{Cl}_{2}\)$$, react with an excess of sodium hydroxide solution at a particular temperature. The reaction produces exactly $$\(35.5 \mathrm{~g}\)$$ of product $$\(\mathbf{X}\)$$. What is product $$\(\mathbf{X}\)$$ ?
A.
\(\mathrm{H}_{2} \mathrm{O}\)
B.
\(\mathrm{NaCl}\)
C.
\(\mathrm{NaClO}\)
D.
\(\mathrm{NaClO}_{3}\)
Exam No：9701_w17_qp_11 Year：2017 Question No：17
Answer:
D
Knowledge points:
11.2.1 describe the relative reactivity of the elements as oxidising agents
11.2.2 describe the reactions of the elements with hydrogen and explain their relative reactivity in these reactions
11.2.3 describe the relative thermal stabilities of the hydrogen halides and explain these in terms of bond strengths
11.3.1 describe the relative reactivity of halide ions as reducing agents
11.3.2.1 aqueous silver ions followed by aqueous ammonia (the formation and formula of the $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$ complex is not required)
11.3.2.2 concentrated sulfuric acid, to include balanced chemical equations
Solution:
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