Term
One mole of particles of any substance contains how many particles?
A)10^6 particles
B) 3 × 10^-10 particles
C) 3 × 10^10 particles
D) 6.02 × 10^23 particles
E) 6.02 × 10^-23particles |
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Definition
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Term
One mole of copper(II) sulfate, CuSO4 , contains ________ moles of O.
A) 4
B) 6.02 × 10 ^23
C) 1.51 × 10^23
D) 2.41 × 10^23
E) 2.41 × 10^24 |
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Definition
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Term
How many moles of carbon atoms are there in 0.500 mole of ?
A) 0.500 mole
B) 1.00 mole
C) 3.00 moles
D) 6.02 × moles
E) 4.00 moles |
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Definition
| 1.00 mole of carbon atoms |
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Term
| What is the molar mass of copper(II) sulfate, CuSO4 ? A) 16.00 g/mole B) 63.60 g/mole C) 111.6 g/mole D) 159.6 g/mole E) 319.2 g/mole |
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Definition
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Term
The molar mass of calcium hydroxide, Ca(OH)2 , is ________.
A) 58.09 g/mole
B) 57.09 g/mole
C) 74.10 g/mole
D) 114.2 g/mole
E) 54.02 g/mole |
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Definition
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Term
How many moles of water, H2O, are present in 75.0 g H2O?
A) 4.41 moles
B) 4.16 moles
C) 75.0 moles
D) 7.50 moles
E) 1.35 × moles |
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Definition
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Term
4.00 moles of sodium have a mass of ________.
A) 4.60 g
B) 11.0 g
C) 23.0 g
D) 44.0 g
E) 92.0 g |
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Definition
| 92.0 g (22.99 g/mol Na)(4.00) |
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Term
How many moles of K2SO4 are in 15.0 g of K2SO4?
A) 0.172 moles
B) 2.61 × 103 moles
C) 0.111 moles
D) 0.0861 moles
E) 0.119 moles |
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Definition
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Term
3.00 moles of NO2 have a mass of ________.
A) 138 g
B) 46.0 g
C) 30.0 g
D) 90.0 g
E) 45.0 g |
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Definition
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Term
For the following question(s), use this equation 2Mg+O2→ 2MgO
10) The number of moles of oxygen gas needed to react with 4.0 moles of Mg is ________.
A) 1.0 mole
B) 2.0 moles
C) 3.0 moles
D) 4.0 moles
E) 6.0 moles |
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Definition
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Term
For the following question(s), use this equation 2Mg+O2→ 2MgO
11) How many grams of magnesium are needed to react with 16 g of O2?
A) 0.50
g
B) 1.0 g
C) 12 g
D) 24 g
E) 48 g |
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Definition
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Term
In the reaction of silver nitrate with sodium chloride, how many grams of silver chloride will be produced from 100. g of silver nitrate when it is mixed with an excess of sodium chloride? The equation for the reaction is below.
AgNO3+NaCl→ AgCl+NaNO3
A) 107.9 g
B) 169.9 g
C) 84.4 g
D) 0.589 g
E) 58.9 g |
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Definition
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Term
When 4 moles of aluminum are allowed to react with an excess of chlorine gas, , how many moles of aluminum chloride are produced?
2Al+3Cl2→2Alcl3
A) 1 mole
B) 2 moles
C) 3 moles
D) 4 moles
E) 5 moles |
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Definition
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Term
) A reaction that releases energy as it occurs is classified as a(n) ________.
A) endothermic reaction
B) exothermic reaction
C) oxidation-reduction reaction
D) catalyzed reaction
E) decomposition reaction |
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Definition
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Term
15) Any reaction that absorbs 150 kcal of energy can be classified as ________.
A) endothermic
B) exothermic
C) activated
D) reduction
E) oxidation |
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Definition
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Term
A chemical equation is balanced when ________.
A) the total number of molecules is the same in reactants and products
B) the total number of ions is the same in reactants and products
C) the sum of the coefficients of the reactants is equal to the sum of the coefficients of the products
D) the number of atoms of each element is the same in reactants and products
E) the charge on each atom is the same in reactants and products |
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Definition
| The number of atoms of each element is the same in reactants and products |
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Term
What coefficient is placed in front of to complete the balancing of the following equation?
C5H8+? O2→5CO2+4H2O
A) 1
B) 3
C) 5
D) 7
E) 9 |
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Definition
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Term
What is the coefficient of hydrogen, H2 when the following equations is balanced?
Al+H2SO4→Al2(SO4)3+ ? H2
A) 1
B) 2
C) 3
D) 4
E) 5 |
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Definition
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Term
In this reaction, what is the correct coefficient for sodium chloride?
Pb(NO3)2+?NaCl→PbCl2+?NaNO3
A) 1
B) 2
C) 3
D) 4
E) 5 |
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Definition
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Term
For the following reaction, what is the correct coefficient for the H2 ?
Fe + HCl → FeCl3 + H2
A) 1
B) 2
C) 3
D) 4
E) 5 |
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Definition
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Term
What is the classification for this unbalanced reaction?
Fe + HCl → FeCl3 + H2
A) combustion
B) combination
C) decomposition
D) single replacement
E) double replacement |
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Definition
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Term
In a ________ reaction, two or more elements or compounds form one product.
A) decomposition
B) single replacement
C) combustion
D) double replacement
E) combination |
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Definition
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Term
The following reaction takes place when an electric current is passed through water. It is an example of a ________ reaction.,
2H2O→→2H2+O2
A) combination
B) single replacement
C) combustion
D) decomposition
E) double replacement |
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Definition
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Term
In an oxidation-reduction reaction, the substance oxidized always ________.
A) takes on oxygen atoms
B) loses electrons
C) gives up hydrogen atoms
D) gains electrons
E) becomes a charged species |
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Definition
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Term
What type of reaction is the following?
2KClO3 → 2KCl + 3O2 |
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Definition
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Term
| The molar mass of water is 18.02 g.( True or False) |
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Definition
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Term
According to the kinetic molecular theory of gases, a gas can be compressed much more than a liquid or solid because ________.
A) a gas is composed of very small particles
B) the particles of a gas are very far apart
C) gas particles move rapidly
D) gas particles do not attract or repel one another
E) gas particles move faster when the temperature increases |
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Definition
| Particles of a gas are very far apart |
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Term
The force of gas particles against the walls of a container is called ________.
A) pressure
B) volume
C) temperature
D) quantity of gas
E) density |
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Definition
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Term
A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?
A) 1.50 mmHg
B) 507 mmHg
C) 760 mmHg
D) 1140 mmHg
E) 3800 mmHg |
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Definition
| 1140 mmHg (forget volume) |
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Term
The volume of a gas with a pressure of 1.2 atm increases from 1.0 L to 4.0 L. What is the final pressure of the gas, assuming constant temperature and amount of gas?
A) 1.2 atm
B) 0.30 atm
C) 3.3 atm
D) 4.8 atm
E) 1.0 atm |
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Definition
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Term
The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming constant temperature and amount of gas?
A) 4100 L
B) 5.0 L
C) 0.0060 L
D) 5.4 L
E) 4.6 L |
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Definition
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Term
What temperature scale is used in gas law calculations?
A) Fahrenheit
B) Celsius
C) Kelvin
D) either Celsius or Fahrenheit
E) either Celsius or Kelvin |
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Definition
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Term
The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure and amount of gas in the container is kept constant?
A) 210 mL
B) 1170 mL
C) 0.00950 mL
D) 0.00474 mL
E) 110 mL |
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Definition
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Term
A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K, if the volume and amount of gas do not change?
A) 1.5 atm
B) 0.94 atm
C) 0.47 atm
D) 2.1 atm
E) 1.1 atm |
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Definition
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Term
At STP, temperature and pressure have the values of ________.
A) 0 K and 1 atm
B) 273 K and 1 mmHg
C) 273 K and 760 mmHg
D) 0 K and 760 mmHg
E) 760 K and 273 atm |
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Definition
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Term
A gas sample contains 4.0 g of CH4 and 2.0 g of He. What is the volume of the sample at STP?
A) 130 L
B) 11 L
C) 17 L
D) 30. L
E) 5.6 L |
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Definition
| 17 L remember: 1 mole gas=22.4 L (STP) |
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Term
How many moles of neon occupy a volume of 14.3 L at STP? A) 36.7 moles B) 32.0 moles C) 6.45 moles D) 0.638 moles E) 1.57 moles |
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Definition
| 0.638 moles → remember: 1 mole gas = 22.4L STP 1mol/22.4L x 14.3 |
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Term
At STP, how many moles of helium would occupy 1.00 L?
A) 2.24 moles
B) 224 moles
C) 22.4 moles
D) 0.446 moles
E) 0.0446 moles |
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Definition
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Term
A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?
A) 2.1 atm
B) 0.55 atm
C) 1.0 × 10^3 atm
D) 1.5 atm
E) 1600 atm |
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Definition
| 1.010.75 or 1.0 x 103 atm |
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Term
| Nitrogen makes up about _________percent of the atmosphere |
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Definition
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Term
| A barometer is usually filled with |
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Definition
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Term
| A temperature of 273°C is equivalent to ______ K |
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Definition
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Term
| The air we breathe is about 21% oxygen. ( True or False) |
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Definition
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Term
| The volume of 1 mole of any gas at STP is 22.4 L ( True or False). |
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Definition
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Term
A hydrogen bond is ________.
A) an attractive force between molecules where partially positive hydrogen atoms are attracted to partially negative atoms of F,O, or N
B) a covalent bond between H and O
C) an ionic bond between H and another atom
D) a bond that is stronger than a covalent bond
E) the polar O—H bond in water |
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Definition
| an attractive force between molecules where partially positive hydrogen atoms are attracted to partially negative atoms of F,O, or N |
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Term
A mixture is prepared by dissolving 2 g of KCl in 100 g of H2O. In this mixture, H2O is the ________. A) solute B) solvent C) solution D) solid E) ionic compound |
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Definition
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Term
Oil does not dissolve in water because ________.
A) oil is polar
B) oil is nonpolar
C) water is nonpolar
D) water is saturated
E) oil is hydrated |
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Definition
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Term
Water is a polar solvent and hexane (C5H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute in the given solvent?
A) mineral oil, soluble in water B) CaCl2 , soluble in hexane C)NaHCO3 , soluble in water D)CCl4 , soluble in water E)octane octane, soluble in water |
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Definition
| NaHCO3 is soluble in water |
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Term
In water, a substance that ionizes completely in solution is called a ________.
A) weak electrolyte
B) nonelectrolyte
C) semiconductor
D) nonconductor
E) strong electrolyte |
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Definition
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Term
) An equivalent is ________.
A) the amount of ion that has a 1+ charge
B) the amount of ion that has a 1- charge
C) the amount of ion that carries 1 mole of electrical charge
D) 1 mole of any ion |
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Definition
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Term
When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is ________.
A) dilute
B) polar
C) nonpolar
D) saturated
E) unsaturated |
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Definition
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Term
An increase in the temperature of a solution usually ________.
A) increases the boiling point
B) increases the solubility of a gas in the solution
C) increases the solubility of a solid solute in the solution
D) decreases the solubility of a solid solute in the solution
E) decreases the solubility of a liquid solute in the solution |
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Definition
| Increases the solubility of a solute in the solution |
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Term
) The mass percent concentration refers to ________.
A) grams of solute in 1 kg of solvent
B) grams of solute in 1 kg of solution
C) grams of solute in 100 g of solvent
D) grams of solute in 100 g of solution
E) grams of solvent in 100 g of solution |
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Definition
| Grams of solute in 100g of solution |
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Term
What is the concentration, in mass percent (m/m), of a solution prepared from 50.0 g NaCl and 150.0 g of water?
A) 0.250% (m/m)
B) 33.3% (m/m)
C) 40.0% (m/m)
D) 25.0% (m/m)
E) 3.00% (m/m) |
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Definition
| 25.0% → g solute/g solution x 100 |
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Term
What is the concentration, mass/volume percent (m/v), of a solution prepared from 50. g NaCl and 2.5 L of water?
A) 5.0% (m/v)
B) 2.0% (m/v)
C) 0.020% (m/v)
D) 0.050% (m/v)
E) 20.% (m/v) |
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Definition
| 2.0 % → g solute/mL solution x 100 (convert L to mL!) |
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Term
What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH?
A) 18 mL
B) 0.13 mL
C) 13 mL
D) 120 mL
E) 8.0 × 10^2mL |
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Definition
| 800 mL or 8.0 x 10^2 ml → g solute/mL solution x 100 |
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Term
What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution?
A) 34 M
B) 2.0 M
C) 0.50 M
D) 0.029 M
E) 1.0 M |
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Definition
| 2.0 M → Molarity = moles of solute/Liter of solution |
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Term
) The molarity (M) of a solution refers to ________.
A) moles of solute/L of solution B) moles of solute/ L of solvent C) moles of solute/100 mL of solution D) grams of solute/100 mL of solution E) grams of solute/L of solution |
|
Definition
| moles of solute / L of solution |
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Term
What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution?
A) 2.5 M
B) 1.0 M
C) 5.0 M
D) 10. M
E) 2.0 M |
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Definition
| 2.0 M → Molarity= moles solute/ L solution |
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Term
What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH?
A) 3.0 L
B) 0.50 L
C) 2.0 L
D) 4.5 L
E) 0.22 L |
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Definition
| 2.0L → Molarity= moles solute/ Volume solution |
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Term
What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?
A) 0.267 M
B) 0.150 M
C) 0.200 M
D) 6.67 M
E) 0.100 M |
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Definition
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Term
| What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution? |
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Definition
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Term
A homogeneous mixture that does not settle out upon standing is ________.
A) an element
B) a colloid
C) a suspension
D) solid
E) hydrated |
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Definition
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Term
A solution with the same osmotic pressure as the blood is ________.
A) isotonic to the blood
B) hypotonic to the blood
C) hypertonic to the blood
D) nontonic to the blood
E) molar to the blood |
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Definition
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Term
Which solution is isotonic to a red blood cell?
A) water
B) 0.5% NaCl
C) 2% glucose
D) 0.9% NaCl
E) 10% glucose |
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Definition
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Term
Acetic acid can be classified as a ________.
A) gas
B) solid
C) weak electrolyte
D) strong electrolyte
E) ionic compound |
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Definition
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Term
Using a kidney machine to remove waste products from the blood is known as ________.
A) osmosis
B) osmolysis
C) autolysis
D) hemolysis
E) hemodialysis |
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Definition
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Term
| Polar solutes are soluble in ________ solvents. |
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Definition
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Term
| A substance that produces only a small number of ions in solution is known as a ________ electrolyte. |
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Definition
|
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Term
| ) The number of moles of a compound dissolved in one liter of a solution is called the ________. |
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Definition
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