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Ch.4 - Chemical Quantities & Aqueous Reactions
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 28
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Chapter 4, Problem 28

Calculate how many moles of NH3 form when each quantity of reactant completely reacts. 3 N2H4(l) → 4 NH3(g) + N2(g), given the following reactant quantities: a. 2.6 mol N2H4, b. 3.55 mol N2H4, c. 4.88 kg N2H4.

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1
<Identify the balanced chemical equation: 3 \text{ N}_2\text{H}_4(l) \rightarrow 4 \text{ NH}_3(g) + \text{ N}_2(g)>
<Determine the mole ratio between \text{N}_2\text{H}_4 and \text{NH}_3 from the balanced equation, which is 3:4.>
<For part a, use the mole ratio to calculate moles of \text{NH}_3: \text{moles of NH}_3 = \frac{4}{3} \times 2.6 \text{ mol N}_2\text{H}_4.>
<For part b, use the mole ratio to calculate moles of \text{NH}_3: \text{moles of NH}_3 = \frac{4}{3} \times 3.55 \text{ mol N}_2\text{H}_4.>
<For part c, first convert 4.88 kg \text{N}_2\text{H}_4 to moles using its molar mass, then use the mole ratio to find moles of \text{NH}_3: \text{moles of NH}_3 = \frac{4}{3} \times \text{moles of N}_2\text{H}_4.>
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Textbook Question

Consider the unbalanced equation for the neutralization of acetic acid: HC2H3O2(aq) + Ba(OH)2(aq) → H2O(l) + Ba(C2H3O2)2(aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 0.461 mole of HC2H3O2.

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Open Question
Calculate how many moles of NO2 form when each quantity of reactant completely reacts. Reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) a. 15.2 g N2O5 b. 6.8 mol N2O5 c. 2.87 kg N2O5
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

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Textbook Question

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

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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.

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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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