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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.3 - Chemical Reactions and Reaction Stoichiometry문제 81a
3장, 문제 81a

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of sodium carbonate are present after the reaction is complete? How many grams of sodium nitrate are present after the reaction is complete?

검증된 단계별 안내
1
Write the balanced chemical equation for the reaction: \[ \text{Na}_2\text{CO}_3 (aq) + 2\text{AgNO}_3 (aq) \rightarrow \text{Ag}_2\text{CO}_3 (s) + 2\text{NaNO}_3 (aq) \]
Calculate the molar mass of sodium carbonate (Na\_2CO\_3) and silver nitrate (AgNO\_3).
Determine the number of moles of sodium carbonate and silver nitrate using their respective masses and molar masses.
Identify the limiting reactant by comparing the mole ratio from the balanced equation with the moles available.
Calculate the amount of sodium carbonate remaining after the reaction by considering the stoichiometry and the limiting reactant.

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주요 개념

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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the amounts of substances consumed and produced in a reaction, using mole ratios derived from the coefficients of the balanced equation.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the remaining quantities of reactants after the reaction has occurred.
추천 영상:
가이드 코스
01:30
Limiting Reagent Concept

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble solid, known as a precipitate. In this case, silver carbonate precipitates out of the solution when sodium carbonate and silver nitrate are mixed, which is essential for understanding the reaction's outcome and the quantities of reactants left.
추천 영상:
가이드 코스
01:53
Selective Precipitation
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교과서 질문

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of sulfuric acid and grams of acetic acid present in the mixture after the reaction is complete.

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교과서 질문

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

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교과서 질문

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (a) Which is the limiting reactant?

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교과서 질문

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of silver carbonate are present after the reaction is complete?

3918
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교과서 질문

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of lead(II) acetate present in the mixture after the reaction is complete.

895
views
교과서 질문

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?

639
views