Use the following balanced equation to 3NO2 + H2O 2 HNO3 + NO 8. How many moles

Question

Use the following balanced equation to 3NO2 + H2O 2 HNO3 + NO 8. How many moles of NO2 are required to react with 4 60 moles of H20? A) 2.46 moles NO2 (B) 13.8 moles NO ) 2.30 moles NO2 D) 153 moles NO mc 9. How many moles of HNO3 are formed when 4.60 moles of H20 react with 4.60 moles o A) 153 moles HNO3 B) 2.30 moles HNO3 on t 3.07 moles HNO3 D) 9.20 moles HNO3 10 Limiting Reactant B) HNO3 C) NO2 Q) NO 11. Give the theoretical yield in grams of HNO3: A) 964 g 8) 145 g 3.07 1939 D) 580 g 12. Give the percent yield when 84.5 g of HNO3 are formed from the reaction. A) 88% B) 58% C) 15% 44%

Explanation / Answer

8)
from reaction,
moles of NO2 required = 3*number of moles of H2O
= 3*4.60 moles
= 13.8 moles
Answer: B

9)
Balanced chemical equation is:
3 NO2 + H2O ---> 2 HNO3 + NO


3 mol of NO2 reacts with 1 mol of H2O
for 4.6 mol of NO2, 1.533 mol of H2O is required
But we have 4.6 mol of H2O

so, NO2 is limiting reagent
we will use NO2 in further calculation

According to balanced equation
mol of HNO3 formed = (2/3)* moles of NO2
= (2/3)*4.6
= 3.067 mol
Answer: C

10)
Answer: A (As found in question 9)

11)
Molar mass of HNO3,
MM = 1*MM(H) + 1*MM(N) + 3*MM(O)
= 1*1.008 + 1*14.01 + 3*16.0
= 63.018 g/mol

use:
mass of HNO3 = number of mol * molar mass
= 3.067*63.02
= 193 g
Answer: C

12)

% yield = actual mass*100/theoretical mass
= 84.5*100/193
= 44%
Answer: D

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