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Chapter 1: Problem 33

Questions 32-36 refer to the following. Two half-cells are set up as follows: Half-Cell A: Strip of \(\mathrm{Cu}(s)\) in \(\mathrm{CuNO}_{3}(a q)\) Half-Cell B: Strip of \(\mathrm{Zn}(s)\) in \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\) (aq) When the cells are connected according to the diagram below, the following reaction occurs: GRAPH CAN'T COPY $$2 \mathrm{Cu}^{+}(a q)+\mathrm{Zn}(s) \rightarrow 2 \mathrm{Cu}(s)+\mathrm{Zn}^{2+}(a q) E^{\circ}=+1.28 \mathrm{V}$$ How many moles of electrons must be transferred to create 127 g of copper? (A) 1 mole of electrons (B) 2 moles of electrons (C) 3 moles of electrons (D) 4 moles of electrons

Short Answer

Expert verified
The correct answer is (B) 2 moles of electrons.

Step by step solution

01

Calculate moles of copper

First, let's work out how many moles of copper correspond to 127 g. The atomic mass of copper (\(Cu\)) is approximately 63.55 g/mol. So, the number of moles can be calculated by dividing the mass in grams by the atomic mass. Therefore, the number of moles of copper is \( \frac{127 g}{63.55 g/mol} = 2\) moles.
02

Apply the stoichiometry of the reaction

In the given reaction, two moles of copper ions (\(Cu^{+}\)) react with one mole of zinc, yielding two moles of copper and one mole of zinc ions (\(Zn^{2+}\)). Each reaction of 1 mole of \( Cu^{+}\) involves the transfer of 1 electron to create 1 mole of \( Cu\). Since we end up with two moles of \( Cu\), we must have transferred 2*1 = 2 moles of electrons.

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Most popular questions from this chapter

\(\mathrm{CaCO}_{3}(s)+2 \mathrm{H}^{+}(a q) \rightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)\) If the reaction above took place at standard temperature and pressure and 150 grams of \(\mathrm{CaCO}_{3}(\mathrm{s})\) were consumed, what was the volume of \(\mathrm{CO}_{2}(g)\) produced at STP? (A) 11 L (B) 22 L (C) 34 L (D) 45 L

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Use the following information to answer questions 14-16 The radius of atoms and ions is typically measured in Angstroms \((A),\) which is equivalent to \(1 * 10^{-10} \mathrm{m} .\) Below is a table of information for three different elements. TABLE NOT AVAILABLE The phosphorus ion is larger than a neutral phosphorus atom, yet a zinc ion is smaller than a neutral zinc atom. Which of the following statements best explains why? (A) The zinc atom has more protons than the phosphorus atom. (B) The phosphorus atom is paramagnetic, but the zinc atom is diamagnetic. (C) Phosphorus gains electrons when forming an ion, but zinc loses them. (D) The valence electrons in zinc are further from the nucleus than those in phosphorus.
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