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Chapter 3: Problem 62

Describe the steps involved in the mole method.

Short Answer

Expert verified
The mole method involves the following steps: writing down the balanced chemical equation, converting known quantities into moles, using stoichiometric ratios from the balanced equation to calculate moles of other substances, and if needed, converting moles back to grams.

Step by step solution

01

Write Down The Balanced Chemical Equation

The first step is to write down the balanced chemical equation of the reaction. All reactants and products, and their stoichiometric coefficients need to be clearly stated.
02

Convert to Moles

If you know the weight of any substance involved, convert this value into moles using the molar mass of the substance (which can be derived from its molecular formula).
03

Use Stoichiometric Ratios

Use the stoichiometric ratios of reactants and products that result from the balanced equation to calculate the moles of other substances. This can be applied to find unknown reactants and products.
04

Convert Back To Grams If Needed

If necessary, especially if the problem asks for solution in grams, convert moles back into grams by multiplying the amount in moles by the substance's molar mass.

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Most popular questions from this chapter

Hydrogen has two stable isotopes, \({ }_{1}^{1} \mathrm{H}\) and \({ }_{1}^{2} \mathrm{H},\) and sulfur has four stable isotopes, \({ }_{16}^{32} \mathrm{~S},{ }_{16}^{33} \mathrm{~S},{ }_{16}^{34} \mathrm{~S},\) and \({ }_{16}^{36} \mathrm{~S}\). How many peaks would you observe in the mass spectrum of the positive ion of hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}^{+}\) ? Assume no decomposition of the ion into smaller fragments.

Peroxyacylnitrate (PAN) is one of the components of smog. It is a compound of \(\mathrm{C}, \mathrm{H}, \mathrm{N},\) and \(\mathrm{O}\). Determine the percent composition of oxygen and the empirical formula from the following percent composition by mass: 19.8 percent \(\mathrm{C}, 2.50\) percent \(\mathrm{H},\) 11.6 percent \(\mathrm{N}\). What is its molecular formula given that its molar mass is about 120 g?

Heating \(2.40 \mathrm{~g}\) of the oxide of metal \(\mathrm{X}\) (molar mass of \(X=55.9 \mathrm{~g} / \mathrm{mol}\) ) in carbon monoxide \((\mathrm{CO})\) yields the pure metal and carbon dioxide. The mass of the metal product is \(1.68 \mathrm{~g}\). From the data given, show that the simplest formula of the oxide is \(\mathrm{X}_{2} \mathrm{O}_{3}\) and write a balanced equation for the reaction.

When heated, lithium reacts with nitrogen to form lithium nitride: $$ 6 \mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Li}_{3} \mathrm{~N}(s) $$ What is the theoretical yield of \(\mathrm{Li}_{3} \mathrm{~N}\) in grams when \(12.3 \mathrm{~g}\) of \(\mathrm{Li}\) are heated with \(33.6 \mathrm{~g}\) of \(\mathrm{N}_{2} ?\) If the actual yield of \(\mathrm{Li}_{3} \mathrm{~N}\) is \(5.89 \mathrm{~g}\), what is the percent yield of the reaction?

When potassium cyanide (KCN) reacts with acids, a deadly poisonous gas, hydrogen cyanide (HCN), is given off. Here is the equation: $$ \mathrm{KCN}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{KCl}(a q)+\mathrm{HCN}(g) $$ If a sample of \(0.140 \mathrm{~g}\) of \(\mathrm{KCN}\) is treated with an excess of \(\mathrm{HCl}\), calculate the amount of \(\mathrm{HCN}\) formed, in grams.
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