Comprehension To find the \( K_{\mathrm{sp}} \) of \( \mathrm{AgBrO}_{3} \), a student prepared ...
0Comprehension
To find the \( K_{\mathrm{sp}} \) of \( \mathrm{AgBrO}_{3} \), a student prepared \( 1 \mathrm{~L} \) of a just saturated solution by adding \( \mathrm{AgBrO}_{3} \) in water at \( 27^{\circ} \mathrm{C} \). \( \mathrm{He} \) found that a copper wire left in the solution overnight became covered with silver and \( \mathrm{Cu}^{2+} \) ions were also formed in the solution. The wire was cleaned, dried and found to weigh \( 6.35 \mathrm{mg} \) less that its original weight.
\[
\mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s}) ; \Delta \mathrm{G}^{0}=-120 \mathrm{~kJ}
\]
The number of moles of \( \mathrm{Cu} \) reacted was
\[
(R=8.0 \mathrm{~J} / \mathrm{K}-\mathrm{mol} ; \mathrm{Cu}=63.5)
\]
(a) \( 1.0 \times 10^{-4} \)
(b) \( 1.0 \)
(c) \( 0.10 \)
(d) \( 1.0 \times 10^{-3} \)
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