Theory Pt. 1
Theory Pt. 2
Stoichiometry
Redox Reactions
Ideal Gasses Math
100
Describe the difference between actual and theoretical yield.
Actual yield: the amount of grams of a substance produced in reality when the reaction occurs and is measured. Always less than the theoretical yield.
Theoretical yield: The amount of grams of a substance produced in theory if there was no loss due to physical constraints.
100
What is the Ideal Gas Law? Describe some of the proportionalities in the equation.
PV=nRT
Inverse: P and V - - - n and T
Direct: P and [n and T] - - - V and [n and T]
100
What is the relationship between moles, mass, and molar mass?
n = m/MM
moles (mol) = mass(g)/molar mass(g/mol)
100
What is the oxidation number for each element in Hg2Cl2?
Hg = +1, Cl = -1
100
Rank the following elements by increasing density at STP if you have a single gram of each (consider elements that are diatomic as gasses as a single atom): Oxygen, Krypton, Hydrogen, Neon, and Calcium.
Hydrogen, Oxygen, Neon, Calcium, and Krypton.
200
What is the Limiting Reagent? Given the moles of each substance (or the means to find them) and the mole ratio of the substances, how do you determine the Limiting Reagent?
The Limiting Reagent is the compound that runs out first and thus limits the amount of product produced.
You determine the limiting reactant by using the number of moles from one substance and transferring that into the number of moles of the other substance using the mole ratio. From there, determine whether there would be an excess or a shortage if all the moles of the substance were to be used.
200
What is a net ionic equation? What must we do to go from a balanced chemical reaction to the equivalent net ionic equation?
A net ionic equation is a "simplified" chemical reaction where only the elements/compounds directly involved in the reaction are shown.
We construct it by splitting up aqueous compounds into ions and then canceling spectator ions that appear unchanged on both sides of the yield sign.
200
H2 (g) + O2 (g) → H2O2 (aq)
4.6826 moles of O2 are reacted with 425.70 grams of H2, 4.0739 moles of H2O2 are produced. What is the percent yield of this reaction?
87.0%
• 100% yield would be 4.68 moles H2O2
• O2 is the limiting reagent
200
Given this chemical reaction:
HI(aq) + LiOH(aq) → LiI(aq) + H2O(l)
select the correct balanced net ionic equation.
H+(aq) + OH-(aq) → H2O(l)
200
A sample of C2H6 experiences a change in pressure from 13900.4 torr to 5.48 atm. During this change, the temperature is also changed from 261 K to 10.4 °C. If its new volume is 4480 cm3, what was its original volume in milliliters?
1240 ml
300
What does the formula [MV = n] represent? Include units in your description.
Formula: Molarity * Volume = Moles
Units: Moles/Liter * Liter = Moles
It describes the relationship between concentration (molarity) and its constituent parts (volume and number of moles).
300
Describe the difference between Oxidation and Reduction. How are they related to the Oxidizing Agent and the Reducing Agent?
Oxidation: The loss of an electron by an ion. It gets more positive. The compound that is oxidized is also the reducing agent.
Reduction: The gaining of an electron by an ion. It gets more negative. The compound that is reduced is also the oxidizing agent.
300
Balance the reaction:
_CO2 + _H2O --> _C2H5OH + _O2
2CO2 + 3H2O --> C2H5OH + 3O2
300
Given this chemical reaction:
V2O5(s) + HCl(aq) → VOCl3(l) + H2O(l)
select the correct balanced net ionic equation.
V2O5(s) + 6Cl-(aq) + 6H+(aq) → 2VOCl3(l) + 3H2O(l)
300
How many grams of C2H3Cl are in a 95.79 L container at 40021.6 torr and 497.3 K?
7726 g
400
What form does a double replacement reaction take? Use variables A, B, C, and D to represent the elements.
k1AB(aq) + k2CD(aq) --> k3AD(s) + k4CB(aq)
400
Describe the ways in which Real Gasses differ from Ideal Gasses.
Real Gasses are not point-like (have volume) and they experience intermolecular forces (attractions and repulsions).
400
Na2CO3 (aq) + HCl (aq) → NaCl (aq) + H2O (l) + CO2 (g)
4.3167 moles of Na2CO3 are reacted with 3.295 moles of HCl, 29.09 grams of H2O are produced. What is the percent yield of this reaction?
98.0%
• 100% yield would be 29.7 grams H2O
• HCl is the limiting reagent
400
Given this chemical reaction:
Mg(s) + H2SO4(aq) → MgSO4(aq) + H2(g)
identify which substance is oxidized and which is reduced.
Mg is oxidized (reducing agent);
H2SO4 is reduced (oxidizing agent)
400
How many moles of Xe are in a 1780 cm3 container at 45676 torr and 779 °C?
1.24 mol
500
Recall and state (to the best of your ability) the six solubility rules shown in class.
500
State all of the gas laws you can remember: Boyle's, Charles', Gay-Lussac's, Avagadro's, combined, and Dalton's.
500
Fe(OH)2 (s) → Fe3O4 (s) + H2O (l) + H2 (g)
If 4.88 moles of H2O are produced, how many moles of Fe(OH)2 were reacted if the reaction proceeds with a 51.4% yield?
14.2 moles Fe(OH)2
• 100% yield would give 9.49 moles H2O
500
Given this chemical reaction:
Pb(s) + AgNO3(aq) → Pb(NO3)2(aq) + Ag(s)
identify the oxidizing agent and the reducing agent.
Pb is oxidized (reducing agent);
AgNO3 is reduced (oxidizing agent)
500
A gaseous mixture of Oxygen and Nitrogen contains 32.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture, if the total pressure is 785.0 mmHg?
0.663 atm