A chemist reacts 8.85 g of iron with an excess of hydrochloric acid to form hydrogen gas and iron (II) chloride. Calculate the theoretical yield and the percent yield of hydrogen if 0.27 g of H2 are collected.

TY = g H2 PY = %

Question

Dirty Harry

Chemistry

26 January, 00:10

A chemist reacts 8.85 g of iron with an excess of hydrochloric acid to form hydrogen gas and iron (II) chloride. Calculate the theoretical yield and the percent yield of hydrogen if 0.27 g of H2 are collected.

TY = g H2 PY = %

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Answers (1)

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Jaxon Santiago · Answer 1

The theoretical yield and percent yield of hydrogen if 0.27 g of H2 collected is calculated as follows

write the reaction equation

that is Fe + Hcl = H2 + FeCl2

calculate moles of Fe = mass/molar mass = 8.85 g/56 g/mol = 0.158 moles

by use mole ratio between Fe : H2 which is 1:1 the theoretical moles of hydrogen = 0.158moles

the theoretical mass is therefore = moles x molar mass

= 0.158 mol x2g/mol = 0.316 grams

% mass = actual mass / theoretical mass x 100

= 0.27/0.316 x100 = 85.4 %

A chemist reacts 8.85 g of iron with an excess of hydrochloric acid to form hydrogen gas and iron (II) chloride. Calculate the theoretical yield and the percent yield of hydrogen if 0.27 g of H2 are collected.TY = g H2 PY = %

A chemist reacts 8.85 g of iron with an excess of hydrochloric acid to form hydrogen gas and iron (II) chloride. Calculate the theoretical yield and the percent yield of hydrogen if 0.27 g of H2 are collected.

TY = g H2 PY = %