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A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCI3). If it is the only product, what mass of PCl3 is formed?

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCI3). If it is the only product, what mass of PCl3 is formed?

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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Could I have help with these two questions homework questions im not really understanding this unit

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃). If it is the only product, what mass of PCl₃ is formed? (Note: There are no graphs or diagrams accompanying this text.)
Transcribed Image Text:A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃). If it is the only product, what mass of PCl₃ is formed? (Note: There are no graphs or diagrams accompanying this text.)
Zinc sulfide reacts with oxygen according to the following chemical equation: \[ 2\text{ZnS}(s) + 3\text{O}_2(g) \rightarrow 2\text{ZnO}(s) + 2\text{SO}_2(g) \] Initially, the reaction mixture contains 5.0 mol of ZnS and 9.0 mol of O₂. Once the reaction has occurred as completely as possible, you need to determine the amount (in moles) of the excess reactant remaining. **Note:** Express your answer in moles to two significant figures. On the website, there is an input interface for the answer with buttons for formatting and submission options.
Transcribed Image Text:Zinc sulfide reacts with oxygen according to the following chemical equation: \[ 2\text{ZnS}(s) + 3\text{O}_2(g) \rightarrow 2\text{ZnO}(s) + 2\text{SO}_2(g) \] Initially, the reaction mixture contains 5.0 mol of ZnS and 9.0 mol of O₂. Once the reaction has occurred as completely as possible, you need to determine the amount (in moles) of the excess reactant remaining. **Note:** Express your answer in moles to two significant figures. On the website, there is an input interface for the answer with buttons for formatting and submission options.
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