When 70. g of Li3N(s) (molar mass 35 g/mol) reacts with excess H2(g), 8.0 g of LiH(s) is produced. The percent yield is closest
1 answer:
The percent yield is closest to 17%
<h3>How to calculate the percentage yield</h3>The reaction between Li3N(s) and LiH(s) is given as:
Calculate the moles of Li3N
Moles = Mass/Molar mass
Moles = 70/35
Moles = 2 moles
From the reaction you can see that 1 mole of Li3N produce 3 moles of LiH, hence the moles of LiH is 6 moles
Determine the mass of LiH (theoretical yield)
Mass of LiH = 6 * 7.95
Mass of LiH = 47.7g
%yield = actual/theoretical * 100
%yield = 8/47.7 * 100
%yiels = 16.77%
Hence the percent yield is closest to 17%
Learn more on percent yield here: brainly.com/question/25996347
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Answer:
0.005 M
Explanation:
Given data:
volume of sample solution ( volume of D ) = 5.0 mL
volume of added stock solution ( V1 ) = 5.0 mL
concentration of added stock solution ( N1 ) = 0.02 M
Total volume of concentration ( V2 )= 10 mL = ( 5.0 mL + 5.0mL)
concentration of Total volume of sample ( C2 ) = 0.01
N2 = ( N1V1 ) / V2
= ( 0.02 * 5 ) / 10 = 0.01 m
absorbance of sample solution ( A1 ) = 0.10
absorbance of additional sample solution ( A2 ) = 0.20
attached below is the remaining part of the detailed solution
