Part D How many molecules (not moles) of NHs are produced from 2.32x10-4 g of H2

Question

Part D How many molecules (not moles) of NHs are produced from 2.32x10-4 g of H2? Express your answer numerically as the number of molecules. Hints Hint 1. How to approach the problem The mass of available hydrogen gas is given in grams. First, convert this mass to moles using the molar mass of hydrogen gas. Use the computed number of moles of hydrogen gas to find the number of moles of ammonia Aroduced in the reaction. Finally, convert the number of moles of ammonia to the number of molecules of ammonia using Avogadro's number. Hint 2. Calculate the number of moles of hydrogen gas (click to open) Hint 3. Calculate the number of moles of ammonia produced (click to open) Ps

Explanation / Answer

D)

Molar mass of H2 = 2.016 g/mol

mass of H2 = 2.32*10^-4 g
mol of H2 = (mass)/(molar mass)
= 2.32*10^-4/2.016
= 1.151*10^-4 mol


we have the Balanced chemical equation as:
N2 + 3 H2 —> 2 NH3


From balanced chemical reaction, we see that
when 3 mol of H2 reacts, 2 mol of NH3 is formed
mol of NH3 formed = (2/3)* moles of H2
= (2/3)*1.151*10^-4 mol
= 7.672*10^-5 mol


Molar mass of NH3 = 1*MM(N) + 3*MM(H)
= 1*14.01 + 3*1.008
= 17.034 g/mol


mass of NH3 = number of mol * molar mass
= 7.672*10^-5*17.034
= 1.31*10^-3 g
Answer: 1.31*10^-3 g

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