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If 1.5 mol of AgNO3(aq) is mixed with 1.0 mol of M8CI2(aq) , how many moles of Mg(NO3)2(aq) will be produced? [ Select ]

If 1.5 mol of AgNO3(aq) is mixed with 1.0 mol of M8CI2(aq) , how many moles of Mg(NO3)2(aq) will be produced? [ Select ]

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The following is a balanced reaction: \[ 2 \text{AgNO}_3 \,(\text{aq}) + \text{MgCl}_2\,(\text{aq}) \rightarrow 2 \text{AgCl} \,(\text{s}) + \text{Mg(NO}_3\text{)}_2\,(\text{aq}) \] ### Explanation: - **Reactants:** - **Silver nitrate (AgNO₃)** in aqueous solution. - **Magnesium chloride (MgCl₂)** in aqueous solution. - **Products:** - **Silver chloride (AgCl)** as a solid (precipitate). - **Magnesium nitrate (Mg(NO₃)₂)** in aqueous solution. This reaction is a typical double displacement reaction, where the ions exchange partners resulting in the formation of an insoluble precipitate (AgCl) and a soluble compound (Mg(NO₃)₂). ### Key Concepts: - **Aqueous (aq):** The substance is dissolved in water. - **Solid (s):** The substance is in solid form, often a precipitate in this type of reaction. - **Balancing Equations:** The number of each type of atom is the same on both sides of the equation, adhering to the law of conservation of mass.
Transcribed Image Text:The following is a balanced reaction: \[ 2 \text{AgNO}_3 \,(\text{aq}) + \text{MgCl}_2\,(\text{aq}) \rightarrow 2 \text{AgCl} \,(\text{s}) + \text{Mg(NO}_3\text{)}_2\,(\text{aq}) \] ### Explanation: - **Reactants:** - **Silver nitrate (AgNO₃)** in aqueous solution. - **Magnesium chloride (MgCl₂)** in aqueous solution. - **Products:** - **Silver chloride (AgCl)** as a solid (precipitate). - **Magnesium nitrate (Mg(NO₃)₂)** in aqueous solution. This reaction is a typical double displacement reaction, where the ions exchange partners resulting in the formation of an insoluble precipitate (AgCl) and a soluble compound (Mg(NO₃)₂). ### Key Concepts: - **Aqueous (aq):** The substance is dissolved in water. - **Solid (s):** The substance is in solid form, often a precipitate in this type of reaction. - **Balancing Equations:** The number of each type of atom is the same on both sides of the equation, adhering to the law of conservation of mass.
**Problem Statement:** If 1.5 mol of AgNO₃(aq) is mixed with 1.0 mol of MgCl₂(aq), how many moles of Mg(NO₃)₂(aq) will be produced? **Answer Options:** There is a dropdown selection box following the problem statement for students to select their answer. **Detailed Explanation:** This question involves a stoichiometry problem using a double displacement reaction: \[ \text{2AgNO}_3(\text{aq}) + \text{MgCl}_2(\text{aq}) \rightarrow \text{2AgCl}(\text{s}) + \text{Mg(NO}_3)_2(\text{aq}) \] Based on the balanced chemical equation: - 2 moles of AgNO₃ react with 1 mole of MgCl₂ to produce 1 mole of Mg(NO₃)₂. - Given 1.5 moles of AgNO₃ and 1.0 mole of MgCl₂: - The reaction is limited by AgNO₃ because it is not present in sufficient quantities to completely react with the available MgCl₂. - Therefore, only 0.75 moles of Mg(NO₃)₂ will be produced (because 1.5 moles of AgNO₃ will produce 0.75 moles of Mg(NO₃)₂).
Transcribed Image Text:**Problem Statement:** If 1.5 mol of AgNO₃(aq) is mixed with 1.0 mol of MgCl₂(aq), how many moles of Mg(NO₃)₂(aq) will be produced? **Answer Options:** There is a dropdown selection box following the problem statement for students to select their answer. **Detailed Explanation:** This question involves a stoichiometry problem using a double displacement reaction: \[ \text{2AgNO}_3(\text{aq}) + \text{MgCl}_2(\text{aq}) \rightarrow \text{2AgCl}(\text{s}) + \text{Mg(NO}_3)_2(\text{aq}) \] Based on the balanced chemical equation: - 2 moles of AgNO₃ react with 1 mole of MgCl₂ to produce 1 mole of Mg(NO₃)₂. - Given 1.5 moles of AgNO₃ and 1.0 mole of MgCl₂: - The reaction is limited by AgNO₃ because it is not present in sufficient quantities to completely react with the available MgCl₂. - Therefore, only 0.75 moles of Mg(NO₃)₂ will be produced (because 1.5 moles of AgNO₃ will produce 0.75 moles of Mg(NO₃)₂).
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