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Chapter 9: Problem 54

Design an experiment to measure the percentage yields for the reactions listed below. If your teacher approves your design, get the necessary materials, and carry out your plan. a. \(\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)\) b. \(2 \mathrm{NaHCO}_{3}(s) \longrightarrow\) $$ \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}_{2}(g) $$ c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow\) $$ \mathrm{CaCO}_{3}(s)+2 \mathrm{NaCl}(a q) $$ d. \(\mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow\) $$ \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$

Short Answer

Expert verified
Plan and perform different methods for each experiment based on the states of reactants and products. For most part, the usage of scale to measure the solid chemicals before and after the reaction provides a reasonable method of measuring yield.

Step by step solution

01

Plan experiment for reaction a

For the reaction \(\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)\), an amount of zinc (Zn) is added into a defined volume of hydrochloric acid (HCl). The product formed is zinc chloride (ZnCl2), and hydrogen gas (H2) which is released. The yield can be measured by weighing the remaining unreacted zinc using a scale and subtracting it from the original amount. The deficit can be accounted as the yield.
02

Plan experiment for reaction b

For the reaction \(2 \mathrm{NaHCO}_{3}(s) \rightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}_{2}(g)\), weigh a specific amount of sodium bicarbonate (NaHCO3) before heating it. After the reaction, the amount of solid sodium carbonate (Na2CO3) formed would be the yield which can be measured by weighing.
03

Plan experiment for reaction c

For the reaction \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow \mathrm{CaCO}_{3}(s)+2 \mathrm{NaCl}(a q)\), an aqueous solution of calcium chloride (CaCl2) is mixed with an aqueous solution of sodium carbonate (Na2CO3). The product calcium carbonate (CaCO3) is a solid which can be filtered and dried. The yield can be determined by weighing the solid product.
04

Plan experiment for reaction d

For the reaction \(\mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\), an aqueous solution of sodium hydroxide (NaOH) is mixed with an aqueous solution of hydrochloric acid (HCl). The yield of water can be measured as the volume increase in the solution after the reaction has been completed.

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Most popular questions from this chapter

How many grams of Al form from 9.73 g of aluminum oxide if the yield is 91\(\% ?\) $$\mathrm{Al}_{2} \mathrm{O}_{3}+3 \mathrm{C} \rightarrow 2 \mathrm{Al}+3 \mathrm{CO}$$

Use the balanced equation below to write mole ratios for the situations that follow. $$2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)$$ \begin{equation}\begin{array}{l}{\text { a. calculating mol } \mathrm{H}_{2} \mathrm{O} \text { given mol } \mathrm{H}_{2}} \\ {\text { b. calculating mol } \mathrm{O}_{2} \text { given mol } \mathrm{H}_{2} \mathrm{O}} \\ {\text { c. calculating mol } \mathrm{H}_{2} \text { given mol } \mathrm{O}_{2}}\end{array}\end{equation}

Assume that 44.3 \(\mathrm{g} \mathrm{Na}_{2} \mathrm{O}\) are formed during the inflation of an air bag. How many liters of \(\mathrm{CO}_{2}(\) density \(=1.35 \mathrm{g} / \mathrm{L})\) are needed to completely react with the \(\mathrm{Na}_{2} \mathrm{O}\) ? $$\mathrm{Na}_{2} \mathrm{O}(s)+2 \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 2 \mathrm{NaHCO}_{3}(s)$$

What mass of oxygen is required to burn 688 g of octane, \(\mathrm{C}_{8} \mathrm{H}_{18},\) completely?

How many grams \(\mathrm{CO}_{2}\) form from the complete combustion of \(1.00 \mathrm{L} \mathrm{C}_{8} \mathrm{H}_{18},\) density 0.700 \(\mathrm{g} / \mathrm{mL} ?\) If only \(1.90 \times 10^{3} \mathrm{g} \mathrm{CO}_{2}\) form, what is the percentage yield?
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