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Chapter 3: Problem 123

Consider the reaction \(3 \mathrm{~A}+2 \mathrm{~B} \rightarrow 3 \mathrm{C}\). A student mixed 4.0 moles of \(\mathrm{A}\) with 4.0 moles of \(\mathrm{B}\) and obtained 2.8 moles of \(\mathrm{C}\). What is the percent yield of the reaction?

Short Answer

Expert verified
The percent yield of the reaction is 70%.

Step by step solution

01

Determine the Limiting Reagent

The reaction shows that 3 moles of \(A\) react with 2 moles of \(B\) to produce 3 moles of \(C\). The given number of moles for \(A\) (4.0 moles) would require \(\frac{4.0 \, \text{moles of A} * 2 \, \text{moles of B}}{3 \, \text{moles of A}} = 2.67 \, \text{moles of B}\). Since we have more \(B\) (4.0 moles) than this, \(A\) is the limiting reagent.
02

Calculate the Theoretical Yield

Based on the balanced equation, 3 moles of \(A\) reacts to give 3 moles of \(C\). Thus, 4.0 moles of \(A\) should theoretically produce \(\frac{4.0 \, \text{moles of A} * 3 \, \text{moles of C}}{3 \, \text{moles of A}} = 4.0 \, \text{moles of C}\). This is the theoretical yield.
03

Calculate the Percent Yield

The percent yield is given by the formula: \(\frac{\text{actual yield}}{\text{theoretical yield}} * 100%\). This gives \(\frac{2.8 \, \text{moles of C}}{4.0 \, \text{moles of C}} * 100% = 70%\).

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Most popular questions from this chapter

Without doing any detailed calculations, arrange the following substances in the increasing order of number of moles: \(20.0 \mathrm{~g} \mathrm{Cl}, 35.0 \mathrm{~g} \mathrm{Br},\) and\(94.0 \mathrm{~g} \mathrm{I}\)

Potash is any potassium mineral that is used for its potassium content. Most of the potash produced in the United States goes into fertilizer. The major sources of potash are potassium chloride \((\mathrm{KCl})\) and potassium sulfate \(\left(\mathrm{K}_{2} \mathrm{SO}_{4}\right) .\) Potash production is often reported as the potassium oxide \(\left(\mathrm{K}_{2} \mathrm{O}\right)\) equivalent or the amount of \(\mathrm{K}_{2} \mathrm{O}\) that could be made from a given mineral. (a) If \(\mathrm{KCl}\) costs \(\$ 0.55\) per \(\mathrm{kg}\), for what price (dollar per \(\mathrm{kg}\) ) must \(\mathrm{K}_{2} \mathrm{SO}_{4}\) be sold to supply the same amount of potassium on a per dollar basis? (b) What mass (in kg) of \(\mathrm{K}_{2} \mathrm{O}\) contains the same number of moles of \(\mathrm{K}\) atoms as \(1.00 \mathrm{~kg}\) of KCl?

Disulfide dichloride \(\left(\mathrm{S}_{2} \mathrm{Cl}_{2}\right)\) is used in the vulcanization of rubber, a process that prevents the slippage of rubber molecules past one another when stretched. It is prepared by heating sulfur in an atmosphere of chlorine:$$\mathrm{S}_{8}(l)+4 \mathrm{Cl}_{2}(g) \longrightarrow 4 \mathrm{~S}_{2} \mathrm{Cl}_{2}(l)$$What is the theoretical yield of \(\mathrm{S}_{2} \mathrm{Cl}_{2}\) in grams when \(4.06 \mathrm{~g}\) of \(\mathrm{S}_{8}\) are heated with \(6.24 \mathrm{~g}\) of \(\mathrm{Cl}_{2} ?\) If the actual yield of \(\mathrm{S}_{2} \mathrm{Cl}_{2}\) is \(6.55 \mathrm{~g}\), what is the percent yield?

A compound containing only \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{Cl}\) was examined in a mass spectrometer. The highest mass peak seen corresponds to an ion mass of 52 amu. The most abundant mass peak seen corresponds to an ion mass of 50 amu and is about three times as intense as the peak at 52 amu. Deduce a reasonable molecular formula for the compound and explain the positions and intensities of the mass peaks mentioned.

What mole ratio of molecular chlorine \(\left(\mathrm{Cl}_{2}\right)\) to molecular oxygen \(\left(\mathrm{O}_{2}\right)\) would result from the breakup of the compound \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) into its constituent elements?
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