IN +3H, ANH,7MILEIn both scenarios depicted graphically,above, the more abundant reactant isthe limiting reactant.Cite evidence and reasoning toexplain how this is possible.Clas|-|ỊCH, K2010-20333333DSAAAACLIS0225The more abundant reactant is the limiting reactant because it doesn'thave enough to fulfill the "recipe." In the first scenario, there needs to be1N2 and 3H2 to make 2NH3. So even though there are 7 H2, only 6 ofthose 7 can be made into 2 2NH3, even though the 1 N2 is already enoughto make an NH3 product. This makes H2 the limiting factor even thoughit's the most abundant. In the second scenario, there has to be 1 CH4 and202 to make the products. With that "recipe," 4 CH4 would need 8 02,but since there are only 6 02, the amount of product that can be made islimited even though 02 is technically the most abundant reactant. Scenario #1How many grams of silver chloride (AgCl) are produced from the reaction between100.0 g of silver nitrate (AgNO,) and 100.0 g barium chloride (BaCl₂) ??2AgNO3(s) + BaCl₂ (s)molesliters100.0 g100 g BaCl2 x100.0 gDetermine the number of moles of product that can be created from 100 g of AgNO₂:100.0 g-AgNO3 x1 mole AgNO3169.87 moles AgNO3What is thelimiting reactant?AgNO3Ba(NO3)2 (5) + 2AgCl (s)0.5887 moles1 moles BaCl2Determine the number of moles of product that can be created from 100 g of BaCl,:2 moles AgC!X1mol Bach208.23 g BaCl2X2 moles AgCl2 moles AgNO30.5887 moles AgCl X 143.2 g AgCl1 mole AgClMOLAR MASSES IF NEEDED:169.87 g/mol143,32 g/mol213.341 g/mol208.23 g/mol0.58868 moles- 200/333.74= 0.5887 moles AgClWhat is the maximum amount ofAgCl that can be formed?AgNO.AgClBa(NO₂)₂200.0/208.23 =84.37 g AgCl0.960476 moles AgCl0.9606 molosAgCl0.5887 moles AgCl

The mass of both AgNO3 and BaCl2 is 100.0 g. The molar mass of AgNO3, BaCl2, and AgCl is 169.87…

Scenario #1 How many grams of silver chloride (AgCl) are produced from the reaction between 100.0 g of silver nitrate (AgNO3) and 100.0 g barium chloride (BaCl₂) ?? 2AgNO3(s) + BaCl2 (s) moles mass liters 100.0 g 100.0 g What is the limiting reactant? AgNO3 Ba(NO3)2 (3) 1 moles BaCl2 208.23 g BaCl2 + Determine the number of moles of product that can be created from 100 g of AgNO: 100.0 g AgNO3 x 1 mole AgNO3 169.87 moles AgNO3 x 2AgCl (s) 0.5887 moles 2 moles AgCl 2 moles AgNO3 Determine the number of moles of product that can be created from 100 g of BaCl₂: 2 moles AgCl 100 g BaCl2 x X Imple Bac12 0.5887 moles AgCI X 143.2 g AgCl 1 mole AgCl 0.58868 moles =200/339.74= 0.5887 moles AgCl MOLAR MASSES IF NEEDED: 169.87 g/mol AgNO, AgCl 143.32 g/mol 213.341 g/mol Ba(NO₂)₂ Back, 208.23 g/mol What is the maximum amount of AgCl that can be formed? 200.0/208.23= 84.37 g AgCl 0.960476 moles AgCl 0.9605 moles AgCl 0.5887 moles AgCl

Scenario #1 How many grams of silver chloride (AgCl) are produced from the reaction between 100.0 g of silver nitrate (AgNO3) and 100.0 g barium chloride (BaCl₂) ?? 2AgNO3(s) + BaCl2 (s) moles mass liters 100.0 g 100.0 g What is the limiting reactant? AgNO3 Ba(NO3)2 (3) 1 moles BaCl2 208.23 g BaCl2 + Determine the number of moles of product that can be created from 100 g of AgNO: 100.0 g AgNO3 x 1 mole AgNO3 169.87 moles AgNO3 x 2AgCl (s) 0.5887 moles 2 moles AgCl 2 moles AgNO3 Determine the number of moles of product that can be created from 100 g of BaCl₂: 2 moles AgCl 100 g BaCl2 x X Imple Bac12 0.5887 moles AgCI X 143.2 g AgCl 1 mole AgCl 0.58868 moles =200/339.74= 0.5887 moles AgCl MOLAR MASSES IF NEEDED: 169.87 g/mol AgNO, AgCl 143.32 g/mol 213.341 g/mol Ba(NO₂)₂ Back, 208.23 g/mol What is the maximum amount of AgCl that can be formed? 200.0/208.23= 84.37 g AgCl 0.960476 moles AgCl 0.9605 moles AgCl 0.5887 moles AgCl

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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