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Chapter 9: Problem 56

What do we mean by the actual yield of a reaction?

Short Answer

Expert verified
The actual yield of a reaction refers to the measured amount of one or more products that is really obtained from the experiment. It can be lower than the theoretical yield, which is the maximum possible amount of product that could be formed based on the balanced chemical equation. The actual yield is influenced by factors such as side reactions, incomplete reactions, or losses during the experimental process.

Step by step solution

01

Understanding chemical reactions and yield #-}

In a chemical reaction, reactants are converted into products. The amount of one or more products that is actually obtained from the reaction is called the yield. There are two types of yields, theoretical yield and actual yield. Theoretical yield is the maximum possible amount of product that could be formed from the limiting reactant, based on the equation, while the actual yield is the measured amount of product that is really obtained from the experiment. Actual yield can be lower than theoretical yield due to factors such as side reactions, incomplete reactions, or losses during the experimental process. It is important to distinguish between these two yields when discussing chemical reactions.

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Most popular questions from this chapter

An organic compound of carbon and hydrogen has the empirical formula CH. What is its molecular formula if its molar mass is: (a) \(26 \mathrm{~g} / \mathrm{mol}\) (b) \(52 \mathrm{~g} / \mathrm{mol}\) (c) \(78 \mathrm{~g} / \mathrm{mol}\)

Calcium reacts with nitrogen gas to form calcium nitride. If \(33.8 \mathrm{~g}\) of calcium react with \(20.4 \mathrm{~g}\) of nitrogen gas, (a) Which reactant is the limiting reagent? (b) If the reaction has a \(72.4 \%\) yield, how many grams of calcium nitride are formed?

Consider the balanced chemical equation $$ \begin{aligned} &\mathrm{Fe}(\mathrm{CO})_{5}(s)+2 \mathrm{PF}_{3}(l)+\mathrm{H}_{2}(g) \rightarrow \\ &\mathrm{Fe}(\mathrm{CO})_{2}\left(\mathrm{PF}_{3}\right)_{2} \mathrm{H}_{2}(s)+3 \mathrm{CO}(g) \end{aligned} $$ (a) How many grams of \(\mathrm{CO}\) could be produced from \(10.0 \mathrm{~g}\) of \(\mathrm{PF}_{3}\), excess \(\mathrm{Fe}(\mathrm{CO})_{5}\), and excess \(\mathrm{H}_{2} ?\) (b) How many grams of \(\mathrm{CO}\) could be produced from \(5.0\) moles of \(\mathrm{Fe}(\mathrm{CO})_{5}, 8.0\) moles of \(\mathrm{PF}_{3}\), and \(6.0\) moles of \(\mathrm{H}_{2}\) ? (c) How many moles of \(\mathrm{CO}\) could be produced from \(25.0 \mathrm{~g}\) of \(\mathrm{Fe}(\mathrm{CO})_{5}, 10.0 \mathrm{~g}\) of \(\mathrm{PF}_{3}\), and excess \(\mathrm{H}_{2} ?\) (d) The density of hydrogen gas at room temperature and atmospheric pressure is \(0.0820 \mathrm{~g} / \mathrm{L}\). When \(5.00 \mathrm{~L}\) of hydrogen gas at room temperature and atmospheric pressure is mixed with excess \(\mathrm{Fe}(\mathrm{CO})_{5}\) and excess \(\mathrm{PF}_{3}\), the mass of \(\mathrm{CO}\) collected is \(13.5 \mathrm{~g}\). What is the theoretical yield (in grams) and the percent yield of \(\mathrm{CO}\) ?

Vitamin \(\mathrm{C}\), also known as ascorbic acid, contains carbon, hydrogen, and possibly oxygen. A \(0.160 \mathrm{~g}\) sample of ascorbic acid is subjected to combustion analysis, yielding \(40.93 \%\) C and \(4.58 \%\) H. If the molar mass of ascorbic acid is approximately \(176 \mathrm{~g} / \mathrm{mol}\), what is its molecular formula?

What is the empirical formula of a compound that is \(17.552 \% \mathrm{Na}, 39.696 \% \mathrm{Cr}\), and \(42.752 \% \mathrm{O} ?\)
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