1. The rate of a chemical reaction normally _ as reactant concentration increase.
2. If a catalyst is used in a reaction the reaction rate _.
Use the following graph to answer questions 23 and 24.
Thermochemistry Test Review
1. Chemical reactions that absorb heat are _.
2. The equation that follows shows the reaction that occurs when hydrochloric acid reacts with
HCl + NaOH H2O + NaCl + 456 kJ
This reaction is _.
3. The equation t
Equilibrium Constant Worksheet
Directions: Write the expression for the equilibrium constant K for the reactions below then solve for K
using the concentrations given. State if products or reactants are favored.
1. N2+ 3H2
[N2] = 0.0200 M
Directions: Indicate shifts by telling what happens to the amount of reactants and
products as a result of shift left and right.
1. N2 + 3H2
2NH3 + heat
Increase concentration o
Chemical Equilibrium and Le Chateliers Principle
Directions: For each gaseous system at equilibrium:
A. Indicate what happens to the equilibrium position when the indicated stress is applied.
B. Tell whether the reaction shifts toward the Left or
Assignment #6: Review and Synthesis
1. What is stated in the Aufbau Principal?
2. What is stated in Hund's Rule?
3. State the Pauli Exclusion Principal.
4. What information is provided by the electron-dot notation?
5. What are valence electrons?
6. What i
1. In what ways is the 4 s orbital of an atom different from a 1s orbital?
2. Write the electron configuration for for Hg.
a. How many electrons are in each level?
b. Which levels are not filled?
3. The electron configuration of carbon is 1s22s22p2. Expla
Mass-Mass Conversions Using a Balanced Equation
1) Barium chloride reacts with silver nitrate to produce barium nitrate and silver
chloride. How many grams of silver chloride can be produced from 31.0 g of
barium chloride reacting with excess silver nitra
Balance the equation, answer the questions:
Magnesium reacts with carbon dioxide to form magnesium oxide and carbon according to
Mg (s) + CO2 (g) -> MgO (s) + C (s)
1. How many moles of Mg react with 1.4 mol of CO2 gas in the react
Assignment #3 (Converting molecules to molecules and volumes to volumes)
Balance the following equations and then answer the questions that follow:
H2 + O 2 H2 O
1. Find the number of molecules of oxygen gas that combine with 10 molecules of
STOICHIOMETRY II UNIT
Assignment #1 (Conversions with compounds)
1. Convert 1.806 x 1023 molecules of Cl2 to moles.
2. Convert 1000 molecules of P4O10 to moles.
3. Convert 360 grams of NH3 (ammonia gas) to moles.
4. How many grams are there in 4.50 moles
1. N2 +3H2 2NH3
How many moles of hydrogen are needed to completely react with two moles of nitrogen?
2. 2KClO3 2KCl + 3O2
How many moles of oxygen are produced by the decomposition of six moles of potassium
1. When propane gas (C3H8) is burned in oxygen gas, carbon dioxide gas and water vapor
are produced along with 2219 kJ of heat energy.
a. Write a balanced chemical equation for this reaction.
b. What is the change in the enthalpy ( H) of the reaction?
a. If 1600 g of sulfur trioxide is released into the environment, how many grams of
sulfuric acid will be formed?
b. How many kJ of heat will be formed if 1600 g of sulfur trioxide are released?
2. 7524 J of energy are used to heat 200 g of water
Unit 13: Thermochemistry Packet
A. Identify and explain endothermic and exothermic reactions, using examples and graphs.
1. In the graph below:
a. determine the change in the enthalpy
b. whether the reaction is endothermic or exothermic
2. Identify the fo
PERCENT COMPOSITION 2
Determine the percent composition of each element in the following compounds.
1. rubidium chloride
2. barium phosphide
3. tin (IV) fluoride
4. cupric bromide
5. aluminum sulfite
6. ammonia (NH3)
7. calcium phosphate
Unit 9 Part 1: Formula Mass, Percent Composition
FORMULA MASS 1
1. Determine the formula mass of the following compounds.
2. Determine the formula mass of the following compounds
Unit 9 Part 2: Empirical and Molecular Formulas
EMPERICAL FORMULA ASSIGNMENT 1
1. An oxide of arsenic contains 3.26 g of arsenic and 1.04 g of oxygen. What is the empirical formula for
2. A sample of sodium oxide weighing 1
Lewis Structures Lab
Draw Lewis Structures for the following molecules. Construct the molecules using the key provided. Have these checked by
your teacher. Predict molecular shape, bond angle and if the molecule is polar or nonpolar.
Black sphere =
Silver is recovered from silver ore by converting the ore into silver sulfate which is then
Phosphoric acid is produced at a fertilizer plant.
Bromine is commercially produced fro
Complete the chemical equations:
_ C3H8 + _ O2 _ CO2 + _ H2O
_NaCl _ Na + _Cl2
_ N2 + _ H2 _NH3
_ H2 + _ O2 _ H2O
Copper ore is decomposed to remove the copper metal
Gasoline is mixed with air in the carburetor and then exploded by a spark in the c
Identify the most likely reaction type and predict the products. If no reaction will occur, then state
No reaction. Balance the equation.
1. _Al + _O2
2. _BaSO4 + _MgCl2
3. _ Zn + _H2SO4
5. _Ba + _S
6. _Ca + _O2