Mole/Mole Ratio
What does the mole ratio allow us to do?
It allows us to convert from moles of one substance in a balanced equation to moles of a second substance.
True or false: The mole ratio is not involved in mass calculations when going from grams of one substance to another substance?
False
Definition of limiting reactant.
The reactant that runs out first and limits the amounts of product that can form.
What is the percent yield formula?
Percent yield = Actual/ Theoretical *100
How many moles of NaF will be produced if 6.7 moles of Na are reacted with excess Na2SiF6?
Na2SiF6 + 4Na → Si + 6NaF
10.05 mol NaF
How many grams of chromium (III) oxide can be produced from 25.0g of solid chromium and excess oxygen? Cr + O2 → Cr2O3
36.54 g Cr2O3
In N2 (g) + 3H2 (g) --> 2NH3 (g), what is the limiting reactant and why?
H2 because the reaction requires 3 moles of H2 and only 1 mole of N2.
What is the definition of theoretical yield?
The maximum amount of a given product that can be formed when the limiting reactant is completely consumed. (amount of product obtained usually calculated)
Actual is usually given in a problem.
Predict the number of moles of CO2 formed when 9.3 moles of propane is burned in excess oxygen.
C3H8 + 5O2 → 3CO2 +4H2O
27.3 mol CO2
What mass of water is needed to completely react with 34g of PCl3?
PCl3 + 3H2O → H3PO3 + 3HCl
13.38 grams H2O
You react 15.0g of A with 15.0g of B. Given the molar mass of A is 15 g/mol, B is 25g/mol, and C is 30g/mol, what will the mass of the product be? A + 3B → 2C
12 grams of C
If we found out that 8.33 grams of Carbon should be produced, and 5.29 g of Carbon was actually made in the lab, what is the percent yield of the reaction?
63.5%
Use the following equation to answer the following questions: N2 + 3H2 → 2NH3,
If 1.00 mole of N2 is produced, how many moles of NH3 would be made?
2 mol NH3
How many grams of tin (ii) fluoride can be produced from 65.0 g of hydrogen fluoride?
Sn + 2HF → SnF2 + H2
254.65 grams SnF2
How many grams of NH3 can be produced from the mixture of 4.98g each of nitrogen and hydrogen? N2 + 3H2 → 2NH3
6.058 g of NH3
Consider the reaction: 2S + 3O2 → 2SO3. Find the percent yield of the product if 2.50 grams of SO3 is produced from 1.50g of O2 and excess sulfur.
100%
Use the following equation to answer the following questions: N2 + 3H2 → 2NH3,
If 0.6 moles of NH3 are produced, how many moles of H2 would be made?
0.9 mol H2
If 175 g of X reacts with diboron trioxide to produce 2.08 moles of B4X3, what element does X represent?
Silicon
Considering the following equation: A + 3B → 4C. If 6.0 moles of A is reacted with 6.0 moles of B, what is the limiting reactant and what would be leftover?
Limiting reactant: B
Excess: A
Consider the reaction: P4 + 6F2 → 4PF3. What mass of P4 is needed to produce 78.0 grams of PF3 if the reaction has a 44.5% yield?
61.75 grams P4