Question

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 to

Answer 1

The percent yield is closest to 17%

How to calculate the percentage yield

The reaction between  Li3N(s) and LiH(s) is given as:
$Li_3N+3H_2\rightarrow 3LiH+NH_3$

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