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WorksheetsStoichiometry Review
Total questions: 25
Worksheet time: 50mins
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
2 NaClO3 (s) → 2NaCl (s) +3 O2 (g)
How many grams of O2 will be produced from 12.00 moles of NaClO3?
256 g of O2
576 g of O2
288 g O2
32 g O2
2H2 + O2 → 2H2O
How many grams of H2O can be produced from 3.91 g of O2?
1.905
4.4
2.2
1.1
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
13.7 mol
2.75 mol
6.11 mol
6.85 mol
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
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.
How many moles of water are in this equation?
0
1
2
can't be determined
Mole Ratios used for conversions are derived from:
the molar mass of the reactants in the balanced chemical equation
the coefficients of the balanced chemical equation
the subscripts of the products in the balanced chemical equation
the group number of each element in the balanced chemical equation
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?
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.
Competing reactions might occur forming other products 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
What does percent yield indicate?
The mass of product that should be obtained
How quickly the reaction is completed
The product of product actually obtained
The efficiency of the chemical reaction
Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?
mass A --> moles A --> moles B --> mass B
moles A --> mass A --> mass B
moles B --> mass A --> mole A --> mass B
moles A --> moles B --> mass B
What is an excess reactant?
The substance that creates a surplus of the reactant after the reaction is complete
The reactant that doesn't get used up as a reactant and is left over
The reactant that is used up first and prevents more from being made
This is another term for a limiting reactant
Say you take a reactant A and calculate the amount of moles of another reactant B required to use up all of A. How do you know which of two reactants is the limiting one?
If the calculated value of B is larger than the amount of A, then B is the limiting reactant.
You compare the calculated amount of B to the actual amount available. If more is required, then A is the limiting reactant. If less is required, then B is the limiting reactant.
If the calculated value of B is larger than the amount of A, then A is the limiting reactant.
You compare the calculated amount of B to the actual amount available. If more is required, then B is the limiting reactant. If less is required, then A is the limiting reactant.
What is a limiting reactant?
The substance that is in excess that doesn't get used up as a reactant.
The reactant that is used up first and prevents more product from being made.
The reactant that makes the product.
The reactant that is used up last and prevents more product from being made.
