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Ch.6 Chemical Reactions: Mole and Mass Relationships
McMurry - Fundamentals of General, Organic, and Biological Chemistry 8th Edition
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoMcMurry 8th EditionCh.6 Chemical Reactions: Mole and Mass RelationshipsProblema 58b
Capitolo 6, Problema 58b

Although Cu is not sufficiently active to react with acids, it can be dissolved by concentrated nitric acid, which functions as an oxidizing agent according to the following equation:
Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O(l)
b. Is 35.0 g of HNO3 sufficient to dissolve 5.00 g of copper?

Guida verificata passo dopo passo
1
Step 1: Write down the balanced chemical equation for the reaction: Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O(l). This equation shows that 1 mole of Cu reacts with 4 moles of HNO3.
Step 2: Calculate the molar mass of Cu and HNO3. For Cu, the molar mass is approximately 63.55 g/mol. For HNO3, the molar mass is approximately 1.01 (H) + 14.01 (N) + 3 × 16.00 (O) = 63.01 g/mol.
Step 3: Convert the given mass of Cu (5.00 g) into moles using the formula: \( \text{moles of Cu} = \frac{\text{mass of Cu}}{\text{molar mass of Cu}} \). Substitute the values to find the moles of Cu.
Step 4: Use the stoichiometric ratio from the balanced equation to determine the moles of HNO3 required to react with the moles of Cu. The ratio is 1 mole of Cu to 4 moles of HNO3. Multiply the moles of Cu by 4 to find the moles of HNO3 needed.
Step 5: Convert the given mass of HNO3 (35.0 g) into moles using the formula: \( \text{moles of HNO3} = \frac{\text{mass of HNO3}}{\text{molar mass of HNO3}} \). Compare the moles of HNO3 available to the moles of HNO3 required to determine if 35.0 g of HNO3 is sufficient to dissolve 5.00 g of Cu.

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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the proportions of substances involved. In this case, stoichiometry will help us find out how much HNO3 is needed to completely react with a given mass of copper.
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Stoichiometry

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For this problem, we need to calculate the molar masses of copper (Cu) and nitric acid (HNO3) to convert the given masses into moles, which is essential for stoichiometric calculations.
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Calculating Molar Mass

Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant in this scenario will allow us to determine if the provided amount of HNO3 is sufficient to dissolve the specified amount of copper.
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Limiting Reagent
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