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WorksheetsCfe Chem
Total questions: 20
Worksheet time: 2hrs 40mins
When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?
90.4%
104%
96.15%
1.04%
Actual yield = 62g
Calculate the percent yield.
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
How many moles of water can be produced if 8 moles H2 are used?
Theoretical yield = 146g
Actual yield = 23.5g
Calculate the percentage yield.
1.16%
116%
25%
34%
Reactant and products might stick to containers, be spilled or inhaled causing actual yield to be less than theoretical yield.
true
false
Competing reactions might occur forming other products causing your actual yield to be less than your theoretical yield.
true
false
Some product may be lost during filtering causing your actual yield to be less than your theoretical yield.
true
false
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
Percent yield=(________)÷(________)×100%
In the image, which reactant is limiting?
The white molecules, because there are extra.
The black atoms, because they are completely used up.
The white molecules, because they are completely used up.
The black atoms, because there are extra.
Atom economy is equal to
Total mass of products / Mass of Reactants
Mass of desired products / Total mass of Reactants
Reactants / Mass of desired products
Total mass of Reactants / Excess reactant
Calculate the atom economy for the Haber process;
N2 + 3H2 --> 2NH3
16.7%
82.3%
85%
100%
Calculate the atom economy for making Calcium Oxide from Calcium Carbonate;
CaCO3 --> CaO + CO2
32%
74%
56%
40%
Calculate the percentage yield if a 2 step industrial process returns a 60% yield in step 1, followed by a 90% yield in step 2
30%
54%
90%
150%
