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Worksheetsmole calculation
Total questions: 28
Worksheet time: 1hrs 24mins
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
Ethane (C2H6) combusts in the above reaction. What is the mole ratio of ethane to oxygen gas?
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
Ethane (C2H6) combusts in the above reaction. What is the mole ratio of carbon dioxide to water?
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
New problem: If 16 moles of carbon dioxide are formed by this reaction, how many moles of water were also produced?
4 mol H2O
6 mol H2O
24 mol H2O
96 mol H2O
384 mol H2O
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
A problem asks how many moles of oxygen gas are needed to react completely with 6 moles of ethane (C2H6). What is the final answer for this problem?
13 mol C2H6
3 mol O2
21 mol O2
42 mol O2
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
New problem: If 3.5 moles of oxygen gas are used up as ethane combusts completely, how many moles of carbon dioxide are produced?
0.5 mol CO2
0.57 mol CO2
2.0 mol CO2
3.0 mol CO2
3.5 mol CO2
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
Which conversion factor should be used to solve the following, "How many moles of argon atoms are present in 11.2 L of argon gas at RTP?"
1 mol = 24 L
How many moles of solute are contained in 3.0 L of a 1.5 mol/dm3 solution?
The formula of iron(II) hydroxide is
FeOH2
FeOH
Fe(OH)2
Fe(OH)3
When reacting Na with Cl2, we calculated that the theoretical yield should be 50 grams. Our actual yield was 20 grams. What is the percent yield?
250%
25%
40%
60%
Theoretical yield = 200g
Actual yield = 150g
Calculate the percent yield.
133%
25%
75%
7.5%
Some product can be transformed completely into energy causing your actual yield to be less than your theoretical yield.
true
false
What is the equation to calculate percent yield?
(Actual yield / Theoretical yield) x 100% = Percent yield
(Theoretical yield / Actual yield) x 100% = Percent yield
Mass (1 Mole / Molar mass) x 100% = Percent yield
Mass x Speed x 100% = Percent yield
A chemical reaction stops before the limiting reagent is used up.
Your percent yield is 50%. The actual amount of product produced was 150 grams. What is the theoretical yield?
30 grams
7.5 grams
75 grams
300 grams
When there is more than one product they are mixed up together, this means that the product produced is ______.
pure
compound
impure
atom
A sample of impure sodium with a purity of 50% is purified to obtain 50g of pure sodium. What was the original mass of the impure sample?
100g
50g
200g
25g
How many grilled cheeses can you make with 26 slices of bread and 14 pieces of cheese?
The reactant that is not completely used up in a chemical reaction is called the __________ .
spectator reagent
limiting reagent
excess reagent
catalyst
1 C10H8 + 12 O2 --> 10 CO2 + 4 H2O
1 Mg + 2 HCl --> 1 MgCl2 + 1 H2
Which reactant is the limiting reagent and why?
2H2(g) + O2(g) → 2H2O(l)
Hydrogen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.
Oxygen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.
