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/molH2O: 18.015 g/molH3PO4: 97.994 g/molHCl; 36.45 g/molWhat is the limiting reagent in this scenario? Note! Make an accurate claim: The limiting reagent in this scenario is _____. Provide additional details and use subject specific language. Cite evidence from what's given to you in the problem that supports your answer, hint: look at that equation!. Lastly! Fully connect the evidence to the claim/your answer to the question. Include subject specific language in your reasoning. Your written response should LOOK similar like the response attached. The other image is there to show how you would figure out the limiting reagent 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 given chemical reaction is PCl5s + 4H2Ol →H3PO4aq + 5HClg. The mass of PCl5 is 12.0 g. The mass…

Answered: In one experiment, 12.0 g of PCl5 was…

Chemistry

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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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Question

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?

Note! Make an accurate claim: The limiting reagent in this scenario is _____. Provide additional details and use subject specific language.

Cite evidence from what's given to you in the problem that supports your answer, hint: look at that equation!. Lastly! Fully connect the evidence to the claim/your answer to the question. Include subject specific language in your reasoning.

Your written response should LOOK similar like the response attached. The other image is there to show how you would figure out the limiting reagent

IN +3H, ANH,
7
MILE
In both scenarios depicted graphically,
above, the more abundant reactant is
the limiting reactant.
Cite evidence and reasoning to
explain how this is possible.
Clas
|-|
ỊCH, K2010-20
333333
DS
AAAA
CL
IS
0
225
The more abundant reactant is the limiting reactant because it doesn't
have enough to fulfill the "recipe." In the first scenario, there needs to be
1N2 and 3H2 to make 2NH3. So even though there are 7 H2, only 6 of
those 7 can be made into 2 2NH3, even though the 1 N2 is already enough
to make an NH3 product. This makes H2 the limiting factor even though
it's the most abundant. In the second scenario, there has to be 1 CH4 and
202 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 is
limited even though 02 is technically the most abundant reactant.

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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