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For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant com- pletely reacts. Assume that there is more than enough of the other reactant.

For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant com- pletely reacts. Assume that there is more than enough of the other reactant.

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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### Educational Chemistry Problems #### Question 32: Sulfuric acid dissolves aluminum metal according to the following reaction: \[ 2 \text{Al}(s) + 3 \text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3 \text{H}_2(g) \] Suppose you want to dissolve an aluminum block with a mass of 15.2 g. - What minimum mass of \(\text{H}_2\text{SO}_4\) (in g) do you need? - What mass of \(\text{H}_2\) gas (in g) does the complete reaction of the aluminum block produce? *Note: Refer to Section 4.3 or watch KCV 4.3 and IWE 4.4 for more details.* #### Question 33: For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. a. \[ \text{Ba}(s) + \underline{\text{Cl}_2}(g) \rightarrow \text{BaCl}_2(s) \] b. \[ \text{CaO}(s) + \underline{\text{CO}_2}(g) \rightarrow \text{CaCO}_3(s) \] c. \[ 2 \text{Mg}(s) + \underline{\text{O}_2}(g) \rightarrow 2 \text{MgO}(s) \] d. \[ 4 \text{Al}(s) + \underline{3 \text{O}_2}(g) \rightarrow 2 \text{Al}_2\text{O}_3(s) \] *Note: Refer to Section 4.3 or watch KCV 4.3 and IWE 4.4 for additional guidance.* #### Question 34: For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume there is more than enough of the other reactant. a. \[ 2 \text{K}(s) + \underline{\text{Cl}_2
Transcribed Image Text:### Educational Chemistry Problems #### Question 32: Sulfuric acid dissolves aluminum metal according to the following reaction: \[ 2 \text{Al}(s) + 3 \text{H}_2\text{SO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3 \text{H}_2(g) \] Suppose you want to dissolve an aluminum block with a mass of 15.2 g. - What minimum mass of \(\text{H}_2\text{SO}_4\) (in g) do you need? - What mass of \(\text{H}_2\) gas (in g) does the complete reaction of the aluminum block produce? *Note: Refer to Section 4.3 or watch KCV 4.3 and IWE 4.4 for more details.* #### Question 33: For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. a. \[ \text{Ba}(s) + \underline{\text{Cl}_2}(g) \rightarrow \text{BaCl}_2(s) \] b. \[ \text{CaO}(s) + \underline{\text{CO}_2}(g) \rightarrow \text{CaCO}_3(s) \] c. \[ 2 \text{Mg}(s) + \underline{\text{O}_2}(g) \rightarrow 2 \text{MgO}(s) \] d. \[ 4 \text{Al}(s) + \underline{3 \text{O}_2}(g) \rightarrow 2 \text{Al}_2\text{O}_3(s) \] *Note: Refer to Section 4.3 or watch KCV 4.3 and IWE 4.4 for additional guidance.* #### Question 34: For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume there is more than enough of the other reactant. a. \[ 2 \text{K}(s) + \underline{\text{Cl}_2
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