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Need help asap In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compounds in the equation are as follows;  PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol What is the limiting reagent in this scenario?   solve the problem Exactly like the example attached.

Need help asap In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compounds in the equation are as follows;  PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol What is the limiting reagent in this scenario?   solve the problem Exactly like the example attached.

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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In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation:

Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g)

The molar masses for each compounds in the equation are as follows; 

PCl5: 208.224 g/mol

H2O: 18.015 g/mol

H3PO4: 97.994 g/mol

HCl; 36.45 g/mol

What is the limiting reagent in this scenario?

 

solve the problem Exactly like the example attached.

Scenario #1 How many grams of silver chloride (AgCl) are produced from the reaction between 100.0 g of silver nitrate (AgNO,) and 100.0 g barium chloride (BaCl₂) ?? 2AgNO3(s) + BaCl₂ (s) moles liters 100.0 g 100 g BaCl2 x 100.0 g Determine the number of moles of product that can be created from 100 g of AgNO₂: 100.0 g-AgNO3 x 1 mole AgNO3 169.87 moles AgNO3 What is the limiting reactant? AgNO3 Ba(NO3)2 (5) + 2AgCl (s) 0.5887 moles 1 moles BaCl2 Determine the number of moles of product that can be created from 100 g of BaCl,: 2 moles AgC! X 1mol Bach 208.23 g BaCl2 X 2 moles AgCl 2 moles AgNO3 0.5887 moles AgCl X 143.2 g AgCl 1 mole AgCl MOLAR MASSES IF NEEDED: 169.87 g/mol 143,32 g/mol 213.341 g/mol 208.23 g/mol 0.58868 moles - 200/333.74= 0.5887 moles AgCl What is the maximum amount of AgCl that can be formed? AgNO. AgCl Ba(NO₂)₂ 200.0/208.23 = 84.37 g AgCl 0.960476 moles AgCl 0.9606 molos AgCl 0.5887 moles AgCl
Transcribed Image Text:Scenario #1 How many grams of silver chloride (AgCl) are produced from the reaction between 100.0 g of silver nitrate (AgNO,) and 100.0 g barium chloride (BaCl₂) ?? 2AgNO3(s) + BaCl₂ (s) moles liters 100.0 g 100 g BaCl2 x 100.0 g Determine the number of moles of product that can be created from 100 g of AgNO₂: 100.0 g-AgNO3 x 1 mole AgNO3 169.87 moles AgNO3 What is the limiting reactant? AgNO3 Ba(NO3)2 (5) + 2AgCl (s) 0.5887 moles 1 moles BaCl2 Determine the number of moles of product that can be created from 100 g of BaCl,: 2 moles AgC! X 1mol Bach 208.23 g BaCl2 X 2 moles AgCl 2 moles AgNO3 0.5887 moles AgCl X 143.2 g AgCl 1 mole AgCl MOLAR MASSES IF NEEDED: 169.87 g/mol 143,32 g/mol 213.341 g/mol 208.23 g/mol 0.58868 moles - 200/333.74= 0.5887 moles AgCl What is the maximum amount of AgCl that can be formed? AgNO. AgCl Ba(NO₂)₂ 200.0/208.23 = 84.37 g AgCl 0.960476 moles AgCl 0.9606 molos AgCl 0.5887 moles AgCl
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