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...

See similar textbooks

Similar questions

Nitrogen monoxide is produced by combustion in an automobile engine. According to the following reaction, how many grams of oxygen gas are necessary to form 0.842 moles nitrogen dioxide?2NO (g) + O2 (g) 2NO2 (g)
Given the unbalanced equation, NH4NO2(s) -> N2(g) + H2O(I), how many grams of H2O are produced from the decomposition of 0.42 g of NH4NO2?
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO: (9) + H2O(1)2 HNO: (1) +NO(9) Suppose that 14 mol NO, and 4 mol H20 combine and react completely. How many moles of the reactant in excess are present after the reaction has completed? O 2 mol H20 O 1 mol NO2 2 mol NO2 O 1 mol H20
A compound is composed of the elements, carbon, hydrogen, and fluorine only. Combustion of the compound produces CO2, H2O, and HFC?H?F? + O2 ➝ CO2 + H2O + HFCombustion of a 5.000 g sample of the compound produces the products shown in the table below. Product Mass (grams) CO2 8.724 H2O 2.143 HF 2.379 Determine the empirical formula for the compound.
What mass of H2 in grams is produced from the reaction if 1.24 mol of H3PO4 was used. EQ : 2Cr + 2H3PO4 -----> 3H2 + 2CrPO4
C3H7OH + 9 O2 -----------> 6 CO2 + 8 H2O How many grams of H2O can be produced when 35.00 g of C3H7OH react with 45.00 g of O2?
11. In mining, roasting is the oxidation of metal sulfides to produce metal oxides and sulfur dioxide, a typical example is zinc sulfide: 2 ZnS + 3 O2 - 2 ZnO + 2 SO2 When 100.0 g of zinc sulfide reacts with 70.0 g of oxygen according to the above reaction, determine: The limiting reagent for the above reaction is? A) ZnS B) ZnO C) SO2 D) O2 E) None of the above
When calcium carbonate reacts with hydrochloric acid, an aqueous solution of calcium chloride, water, and carbon dioxide gas is produced. CaCO3 + 2HCI-CaClna + H,Ony + COte If 0.68 g hydrochloric acid reacts with excess calcium carbonate, what mass of calcium chloride will be produced?
Give the structure corresponding to following IUPAC name. 4-ethyl-1,2-dimethylcyclohexane
3. 4 Al + 3 MnO22 Al2O3 + 3 Mn If 1.528 moles of MnO2 are reacted, how many moles of Al2O3 will be produced?
The equation for the reaction between calcium carbonate and hydrochloric acid is shown. CaCO3(s) + 2HC1(aq) → CaCl2(aq) + H20(1) + CO2(g) How many moles of calcium carbonate will give 24 cm3 of carbon dioxide wh with an excess of the acid? reacted A 1 mol 0.1 mol C 0.01 mol
What is the theoretical yield of HCI if 30.0 g of BCI3 and excess H20 are reacted according to the following balanced reaction? BC13(g) +3 H20(1) H3BO3(s) + 3 HCI(g) The following molar masses are: HCI = 36.46 g/mol BCI3 = 117.17 g/mol %3D H20 = 18.02 g/mol 75.9 g HCI 132 g HCI 187 g HCI 56.0 g HCI 28.0 g HCI