Textbook Question
Calculate how many moles of NO2 form when each quantity of reactant completely reacts. 2 N2O5( g) → 4 NO2(g) + O2(g) a. 2.5 mol N2O5
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 28c
Calculate how many moles of NH3 form when each quantity of reactant completely reacts. 3 N2H4(l) → 4 NH3(g) + N2(g) c. 65.3 g N2H4
Verified step by step guidance1
Identify the balanced chemical equation: \(3 \text{N}_2\text{H}_4 (l) \rightarrow 4 \text{NH}_3 (g) + \text{N}_2 (g)\).
Calculate the molar mass of \(\text{N}_2\text{H}_4\) by adding the atomic masses of nitrogen and hydrogen: \(2 \times 14.01 + 4 \times 1.01\).
Convert the given mass of \(\text{N}_2\text{H}_4\) to moles using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).
Use the stoichiometry of the balanced equation to find the moles of \(\text{NH}_3\) produced. According to the equation, 3 moles of \(\text{N}_2\text{H}_4\) produce 4 moles of \(\text{NH}_3\).
Calculate the moles of \(\text{NH}_3\) by multiplying the moles of \(\text{N}_2\text{H}_4\) by the ratio \(\frac{4}{3}\).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows us to calculate the amount of product formed or reactant consumed based on balanced chemical equations. In this case, the stoichiometric coefficients from the balanced equation indicate the mole ratio between N2H4 and NH3, which is essential for determining how many moles of NH3 can be produced from a given mass of N2H4.
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Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule. To find out how many moles of N2H4 are present in 65.3 g, one must first calculate the molar mass of N2H4, which is crucial for converting grams to moles in stoichiometric calculations.
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Balanced Chemical Equation
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It ensures the law of conservation of mass is upheld. In the given reaction, the balanced equation shows that 3 moles of N2H4 produce 4 moles of NH3, providing the necessary ratios to calculate the moles of NH3 formed from the moles of N2H4 used.
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Related Practice
Textbook Question
Consider the balanced equation:
SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g)
Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.
Textbook Question
Consider the balanced equation:
SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g)
Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.
Textbook Question
Hydrobromic acid dissolves solid iron according to the reaction:
Fe(s) + 2 HBr(aq) → FeBr2(aq) + H2(g)
What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?
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