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57 Cards in this Set

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When an oxidation-reduction reaction occurs, there must be a transfer of
a. electrons
b. neutrons
c. protons
d. ions
Given the reaction:
Cl(g) + Cl(g) --> Cl2(g) + energy
Which statement best describes the reaction?
a. A bond is formed and energy is absorbed.
b. A bond is formed and energy is released.
c. A bond is broken and energy is absorbed.
d. A bond is broken and energy is released.
If equal volumes of 0.1 M NaOH and 0.1 M HCl are mixed, the resulting solution will contain a salt and
a. HCl
b. NaOH
c. H2O
d. NaCl
Which reaction occurs when equivalent quantities of H+ (or H3O+) and OH- are mixed?
a. oxidation
b. reduction
c. hydrolysis
d. neutralization
When butane burns in an excess of oxygen, the principal products are
a. CO2 and H2O
b. CO2 and H2
c. CO and H2O
d. CO and H2
Which reaction represents the process of neutralization?
a. Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g)
b. HCl(aq) + KOH(aq) --> KCl(aq) + H2O(l)
c. Pb(NO3)2(aq) + CaCL2 --> Ca(NO3)2(aq) + PbCl2(s)
d. 2KClO3(s) --> 2KCl(s) + 3O2(g)
How many moles of solute are contained in 200 milliliters of a 1M solution?
a. 1
b. 0.2
c. 0.8
d. 200
Use the following equation to answer the question:
Energy + 2C + 3H2 gives C2H6

On the right hand side of the equation are two carbons and six hydrogens. On the left hand side are two carbons and six hydrogens. This is because:
a. Only two carbons can react with six hydrogens.
b. The conservation of matter is reflected in this model.
c. The conservation of volume is reflected in this model.
d. The formation of ethane requires small amounts of energy.
e. The formation of ethane requires large amounts of energy.
If an equation is balanced properly, both sides of the equation must have the same number of
a. atoms
b. coefficients
c. molecules
d. moles of molecules
Which equation is correctly balanced?
a. H2 + Os --> H2O
b. Ca + Cl2 --> CaCl
c. 2H2 + O2 --> 2H2O
d. Ca + Cl2 --> Ca2Cl
Given the balanced equation:
2Na + S --> Na2S
What is the total number of moles of S that reacted when 4.0 moles of Na were completely consumed?
a. 1.0 mole
b. 2.0 moles
c. 0.5 mole
d. 4.0 moles
Given the unbalanced equation:
__Al(s) + __O2(g) --> __Al2O3(s)
When this equation is correctly balanced using smallest whole numbers, what is the coefficient of O2(g)?
a. 6
b. 2
c. 3
d. 4
Given the reaction:
C6H12O6(s) + 6O2 (g) --> 6CO2(g) + 6H2(l)
How many moles of C6H12O6 are needed to produce 24 moles of carbon dioxide?
a. 1.0 moles
b. 12 moles
c. 24 moles
d. 4.0 moles
Given the unbalanced equation:
__Mg(ClO3)2(s) --> __MgCl2(s) + __O2(g)
What is the coefficient of O2 when the equation is balanced correctly using the smallest whole-number coefficients?
a. 1
b. 2
c. 3
d. 4
Given the reaction:
6CO2 + 6H2 --> C6H12O6 + 6O2
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a. 2.5
b. 6.0
c. 12
d. 15
Given the unbalanced equation:
__Al + __CuSO4 --> __Al2(SO4)3 + __Cu
When the equation is balanced using the smallest whole-number coefficients, what is the coefficient of Al?
a. 1
b. 2
c. 3
d. 4
2C2H2(g) + 5O2(g) --> 4CO2(g) + 2H2O(g)
How many moles of oxygen are required to react completely with 1.0 mole of C2H2?
a. 2.5
b. 2.0
c. 5.0
d. 10
Given the unbalanced equation:
__Fe203 + __CO --> __Fe + __C02
When the equation is correctly balanced using the smallest whole-number coefficients, what is the coefficient of CO?
a. 1
b. 2
c. 3
d. 4
Use the periodic table to find the molar mass for Na2SO4.
a. 22.99 grams/mole
b. 71.05 grams/mole
c. 119.05 grams/mole
d. 142.04 grams/mole
e. 149.03 grams/mole
Using the periodic table find the molar mass for A12(S04)3.
a. 26.98 grams/mole
b. 75.04 grams/mole
c. 123.04 grams/mole
d. 150.02 grams/mole
e. 278.01 grams/mole
What are the coefficients needed to balance the following chemical equation?
N2 + H2 --> NH3
a. 1, 2, 3
b. 1, 3, 2
c. 1, 3, 3
d. 2, 2, 3
e. 2, 3, 2
What are the coefficients needed to balance the following equation?
Fe + 02 --> Fe203
a. 2, 3, 1
b. 2, 6, 2
c. 3, 3, 2
d. 4, 2, 3
e. 4, 3, 2
What are the correct coefficients to balance the equation?
Al(NO3)3 + H2S04 --> A12(S04)3 + HNO3
a. 2, 2, 3, 3
b. 2, 3, 3, 2
c. 2, 3, 1, 6
d. 3, 2, 4, 3
e. 3, 2, 3, 2
A student is ask to balance the chemical equation:
NaOH + H2S04 --> Na2SO4 + H20
He does this by putting a 2 after the Na in NaOH. Is this a correct way to balance an equation? Why?
a. No, because that changes the compound NaOH.
b. No, because the 2 should go behind the OH.
c. Yes, this is the easiest way to balance it.
d. Yes, it doesn't matter where the number goes.
e. Yes, because that changes the compound NaOH.
A student is asked to balance the chemical equation:
Ca(OH)2 + HCI --> CaCI2 + H20
He does this by removing the 2 after the OH and after the Cl. Is this the correct way to balance an equation? Why?
a. No, the numbers should be changed to 3's.
b. No, changing the number changes the compounds.
c. No, a 2 should be put in between H and Cl in HCI.
d. Yes, this is the easiest way to balance equations.
e. Yes, it doesn't matter where the numbers go.
Given: Becky is conducting an experiment in which she measures 30 ml of an acid of unknown concentration. She adds an indicator solution to it, then slowly adds a basic solution of a known concentration from a buret until the acid solution is neutralized. She measure and records the pH of the solution periodically throughout the experiment.

What laboratory technique is Becky using?
a. electrolysis
b. distillation
c. titration
d. electrophoresis
Which reaction would fit this experiment?
a. CuSO4 + 2NaCl --> Na2SO4 + CuCl2
b. 2H2O --> 2H2 + O2
c. KOH + HCl --> H2O + KCl
d. 2H2O + BaSO4 --> H2SO4 + Ba(OH) 2
e. All of the reactions listed.
All bonds holding atoms together within both the reactants and products in Becky’s experiment are of what type?
a. Metallic
b. Ionic
c. Covalent
d. Ionic and Covalent
e. Hydrogen
An oxidation-reduction reaction is set up so that both half-reactions take place in separate beakers that are connected by a salt bridge and an external conductor. A path for the transfer of ions is provided by the
a. anode
b. cathode
c. salt bridge
d. external conductor
An oxidation half-reaction always involves the
a. gain of electrons
b. gain of protons
c. loss of electrons
d. loss of protons
Given the electrochemical cell reaction:
Zn(s) + Ni2(aq) --> Zn2+(aq) + Ni(s)
Which species is oxidized?
a. Zn
b. Ni2+
c. Zn2+
d. Ni
As an electrochemical cell approaches equilibrium, the electrical energy supplied by the cell
a. decreases
b. increases
c. remains the same
Which component of an electrochemical cell is correctly paired with its function?
a. external conductor Ñ allows the solutions to mix
b. external conductor Ñ permits the migration of ions
c. salt bridge Ñ allows the solutions to mix
d. salt bridge Ñ permits the migration of ions
Magnesium reacts with oxygen to form magnesium oxide according to the following equation:
2Mg(s) + O2(g) Í 2MGO(S)
If 0.81 grams of magnesium oxide are formed, how many grams of oxygen reacted?
a. .020 grams 02
b. .025 grams 02
c. .81 grams 02
d. .0 10 grams 02
e. 0.40 grams 02
Use the following equation to answer the question:
Energy + 2C + 3H2 C2H6
carbon hydrogen ethane
On the right hand side of the equation are two carbons and six hydrogens. On the left hand side are two carbons and six hydrogens. This is because:
a. Only two carbons can react with six hydrogens
b. The conservation of matter is reflected in this model.
c. The conservation of volume is reflected in this model.
d. The formation of ethane requires small amounts of energy.
e. The formation of ethane requires large amounts of energy.
Given the equation:
H2(g) + Cl2(g) --> 2HCl(g)
What is the total number of moles of HCl(g) produced when 3 moles of H2(g) is completely consumed?
a. 5 moles
b. 2 moles
c. 3 moles
d. 6 moles
Salt A and salt B were each dissolved in separate beakers of water at 21¡C. The temperature of the salt A solution decrease, and the temperature of the sat B solution increased. Based on these results, which conclusion is correct?
a. The water gained energy from both salt A and salt B.
b. The water lost energy to both salt A and salt B.
c. The water gained energy from salt A and lost energy to salt B.
d. The water lost energy to salt A and gained energy from salt B.
Which phase change is accompanied by the release of heat?
a. H2O(s) --> H2O(g)
b. H2O(s) --> H2O(l)
c. H2O(l) --> H2O(g)
d. H2O(l) --> H2O(s)
Given the reaction:
H2O (l) + 68.3 kcal H2(g) + 1/2 O2(g)
Which statement describes the reverse reaction?
a. It is endothermic and releases energy.
b. It is endothermic and absorbs energy.
c. It is exothermic and releases energy.
d. It is exothermic and absorbs energy.
The burning of magnesium involves a conversion of
a. chemical energy to mechanical energy
b. chemical energy to heat energy
c. heat energy to chemical energy
d. heat energy to mechanical energy
The burning of a match is common example of a chemical reaction. What happens to most of the energy in the match when it burns?
a. It is transformed into the potential energy of heat and light
b. It is transformed into carbon dioxide and water
c It is transformed into ash and smoke
d. It is transformed into kinetic energy of heat and light
e. There is no change in the forms of energy
Which term describes a reaction in which heat is part of the product?
a. cosmothermic
b. endothermic
c. exothermic
d. isothermic
e. nonthermic
Which term describes a reaction in which heat is part of the reactants?
a. cosmothermic
b. endothermic
c. exothermic
d. isothermic
e. nonthermic
A student observed that when sodium hydroxide was dissolved in water, the temperature of the water increased. The student should conclude that the dissolving of sodium hydroxide
a. is endothermic
b. is exothermic
c. produces an acid solution
d. produces a salt solution
When ammonium chloride crystals are dissolved in water, the temperature of the water decreases. What does the temperature change indicate about the dissolving of ammonium chloride in water?
a. It is an endothermic reaction because it absorbs heat.
b. It is an endothermic reaction because it releases heat.
c. It is an exothermic reaction because it absorbs heat.
d. It is an exothermic reaction because it releases heat.
Which phase change is exothermic?
a. solid to liquid
b. solid to gas
c. liquid to solid
d. liquid to gas
Which statement correctly describes this reaction?
a. It is endothermic and energy is absorbed.
b. It is endothermic and energy is released.
c. It is exothermic and energy is absorbed.
d. It is exothermic and energy is released.
Using a jar with a tight fitting lid, a student mixes 2.00 grams of calcium metal and 100 ml of water; the lid is placed on the bottle. The calcium dissolves and gas bubbles rise to the surface of the liquid. What do you predict has happened to the mass of the of the material inside the jar?
a. The mass has decreased.
b. The mass has increased.
c. The mass has not changed.
d. The mass is now 98 grams.
e. The mass is now 100 grams.
Using a container that will seal so that no gas can escape, as student places 5.00 grams of calcium metal and 150 ml of hydrochloric acid. The metal dissolves and gas bubbles rise to the surface of the liquid. What do you predict has happened to the mass of the material inside the container?
a. The mass is 145 grams.
b. The mass is 155 grams.
c. The mass has decreased.
d. The mass has increased.
e. The mass has not changed.
John knew that magnesium (Mg) is a more reactive metal than silver (Ag) after performing a series of chemical reactions. After doing some Internet research, he found the half-cell reduction potentials for the two metals to be:
Mg+2 + 2e- ¨ Mg potential: -2.37 volts
Ag+ + 1e- ¨ Ag potential: +0.80 volts

What is the source of electrons in this cell?
a. The magnesium metal piece.
b. The magnesium nitrate solution.
c. The potassium nitrate solution.
d. The silver nitrate solution.
e. The silver metal piece.
What is the expected voltage output of the cell?
a. 3.17 volts
b. 2.37 volts
c. 1.57 volts
d. 0.80 volts
e. 0.00 volts
What would be the expected voltage output from the cell if the water in the potassium nitrate solution were allowed to evaporate?
a. 3.17 volts
b. 2.37 volts
c. 1.57 volts
d. 0.80 volts
e. 0.00 volts
John knew that aluminum (Al) is a more reactive metal than copper (Cu) after performing a series of chemical reactions. After doing some Internet research, he found the half-cell reduction potentials for the two metals to be:
Al+3 + 3e- Í Al potential: -1.66 volts
Cu+ + 1e- +Í Cu potential: +0.52 volts

What is the source of electrons in this cell?
a. The copper metal piece.

b. The copper I nitrate solution.
c. The potassium nitrate solution.
d. The aluminum nitrate solution.
e. The aluminum metal piece.
What is the expected voltage output of the cell?
a. 2.18 volts.
b. 1.66 volts.
c. 1.14 volts.
d. 0.52 volts.
e. 0.00 volts.
What would be the expected voltage output from the cell if the water in the potassium nitrate solution were allowed to evaporate?
a. 2.18 volts.
b. 1.66 volts.
c. 1.14 volts.
d. 0.52 volts.
e. 0.00 volts.
5.0 mL of liquid A are reacted with 5.0 ml of liquid B and 10.6 ml of product C are formed, From this information, has mass been conserved? Explain the correct answer:
Can't tell. The measurements are in mL, which do not measure mass. Distinguishes between volume and mass (3 pt).
2.00 g of oxygen (02) combine exactly with 0.25 g of hydrogen (H2) to form water (H20).

a. What would you predict the mass of the water to be? (6 points)
b. Which of the three basic laws of chemistry are you applying? (3 points)
c. Explain why this law applies to this situation. (3 points)
2.25 g
law of conservation of mass.
matter is neither created nor destroyed, thus the mass of the water must be the sum of the oxygen and hydrogen.