Open Question
We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution is needed to precipitate all the Cl- ions in the solution as AgCl?
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 27
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
Verified step by step guidance1
<Step 1: Identify the balanced chemical equation. The reaction given is 2 N2O5(g) → 4 NO2(g) + O2(g). This tells us that 2 moles of N2O5 produce 4 moles of NO2.>
<Step 2: For part (a), convert the mass of N2O5 to moles. Use the molar mass of N2O5, which is approximately 108.01 g/mol. Calculate the moles of N2O5 by dividing the given mass (15.2 g) by the molar mass.>
<Step 3: Use the stoichiometry of the reaction to find the moles of NO2 produced. From the balanced equation, 2 moles of N2O5 produce 4 moles of NO2. Use this ratio to convert moles of N2O5 to moles of NO2.>
<Step 4: For part (b), directly use the given moles of N2O5 (6.8 mol) and apply the stoichiometric ratio from the balanced equation to find the moles of NO2.>
<Step 5: For part (c), convert the mass of N2O5 from kilograms to grams (2.87 kg = 2870 g). Then, follow the same process as in Step 2 to convert grams to moles, and use the stoichiometric ratio to find the moles of NO2.>
Related Practice
Open Question
Consider the unbalanced equation for the combustion of hexane: C6H14(g) + O2(g) → CO2(g) + H2O(g). Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.
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.
1998
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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
6124
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Open Question
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.
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
1681
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