Six mole-to-mole conversion factors has to be written that can be derived from the chemical equation 2 H 2 O 2 → 2 H 2 O + O 2 . Concept Introduction: The coefficients that are present in a balanced chemical equation is like subscripts in the chemical formula. These coefficients can be interpreted in two levels. One is a microscopic level and another is macroscopic level. Microscopic level: The coefficients that are present in a balanced chemical equation gives numerical relationship between the formula units consumed or produced when a chemical reaction takes place. Macroscopic level: In a balanced chemical equation, the coefficients gives information about the fixed molar ratios among the substance that is consumed or produced when a chemical reaction takes place.

Question

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol

Answer 1

Question

Chapter 6, Problem 6.60EP

Interpretation Introduction

Interpretation:

Six mole-to-mole conversion factors has to be written that can be derived from the chemical equation 2H2O2 → 2H2O + O2.

Concept Introduction:

The coefficients that are present in a balanced chemical equation is like subscripts in the chemical formula. These coefficients can be interpreted in two levels. One is a microscopic level and another is macroscopic level.

Microscopic level:

The coefficients that are present in a balanced chemical equation gives numerical relationship between the formula units consumed or produced when a chemical reaction takes place.

Macroscopic level:

In a balanced chemical equation, the coefficients gives information about the fixed molar ratios among the substance that is consumed or produced when a chemical reaction takes place.

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Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) Calculate the number of moles of AgNO3 produced by the reaction of 2.85 moles of Ag with excess HNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol.

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) Calculate the number of moles of AgNO3 produced by the reaction of 109.31 grams of Ag with excess HNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol.