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Chemistry
Q:
Which of the following regions of the electromagnetic spectrum has the lowest frequency?
A.x-ray
B.gamma ray
C.ultraviolet
D.infrared
E.visible
Q:
Which of the following regions of the electromagnetic spectrum have longer wavelengths than visible light?
1/ infrared radiation
2/ ultraviolet radiation
3/ microwave radiation
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1 and 3
Q:
Internal energy and enthalpy are state functions. What is meant by this statement?
Q:
Why are you at greater risk from being burned by steam at 100 C than from liquid water at the same temperature?
Q:
Dry ice converts directly from a solid to a gas when heated. This process is called ________.
Q:
The heat required to convert a solid at its melting point to a liquid is called the heat of ________.
Q:
In thermodynamics, a(n) ________ is defined as the object, or collection of objects, being studied. The surroundings include everything else.
Q:
The standard molar enthalpy of formation of NH3(g) is -45.9 kJ/mol. What is the enthalpy change if 9.51 g N2(g) and 1.96 g H2(g) react to produce NH3(g)?A.-10.3 kJ/mol-rxnB.-20.7 kJ/mol-rxnC.-29.8 kJ/mol-rxnD.-43.7 kJ/mol-rxnE.-65.6 kJ/mol-rxn
Q:
The standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ.C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g)Calculate DfH for propane based on the following standard molar enthalpies of formation.molecule DfH (kJ/mol-rxn)CO2(g) -393.5H2O(g) -241.8A.-1407.7 kJ/mol-rxnB.+104.7 kJ/mol-rxnC.-104.7 kJ/mol-rxnD.-4190.7 kJ/mol-rxnE.+1407.7 kJ/mol-rxn
Q:
Calculate DrH for the combustion of ammonia,4 NH3(g) + 7 O2(g) 4 NO2(g) + 6 H2O()using standard molar enthalpies of formation.molecule DfH (kJ/mol-rxn)NH3(g) -45.9NO2(g) +33.1H2O() -285.8A.+30.24 kJ/mol-rxnB.-206.9 kJ/mol-rxnC.-298.6 kJ/mol-rxnD.-1398.8 kJ/mol-rxnE.-1663.6 kJ/mol-rxn
Q:
Calculate DfH for sulfur dioxide given the thermochemical equations below.2 S(s) + 3 O2(g) 2 SO3(g) DrH = -791.5 kJ/mol-rxn2 SO2(g) + O2(g) 2 SO3(g) DrH = -197.9 kJ/mol-rxnA.-296.8 kJ/mol-rxnB.-395.7 kJ/mol-rxnC.-494.7 kJ/mol-rxnD.-593.6 kJ/mol-rxnE.-989.4 kJ/mol-rxn
Q:
Which of the following chemical equations does not correspond to a standard molar enthalpy of formation?
A.Mg(s) + C(s) + 3/2 O2(g) MgCO3(s)
B.C(s) + 1/2 O2(g) CO(g)
C.N2(g) + O2(g) 2 NO(g)
D.N2(g) + 2 O2(g) N2O4(g)
E.H2(g) + 1/2 O2(g) H2O()
Q:
Which of the following chemical equations corresponds to the standard molar enthalpy of formation of Na2CO3(s)?
A.2 Na(s) + C(s) + 3 O(g) Na2CO3(s)
B.Na2O(s) + CO2(g) Na2CO3(s)
C.Na2(s) + C(s) + 3 O(g) Na2CO3(s)
D.Na2O2(s) + CO(g) Na2CO3(s)
E.2 Na(s) + C(s) + 3/2 O2(g) Na2CO3(s)
Q:
Determine the standard enthalpy of formation of calcium carbonate from the thermochemical equations given below.
Ca(OH)2(s) CaO(s) + H2O() DrH = 65.2 kJ/mol-rxn
Ca(OH)2(s) + CO2(g) CaCO3(s) + H2O() DrH = -113.8 kJ/mol-rxn
C(s) + O2(g) CO2(g) DrH = -393.5 kJ/mol-rxn
2 Ca(s) + O2(g) 2 CaO(s) DrH = -1270.2 kJ/mol-rxn
A.-1712.3 kJ/mol-rxn
B.-441.8 kJ/mol-rxn
C.-849.6 kJ/mol-rxn
D.-980.6 kJ/mol-rxn
E.-1207.6 kJ/mol-rxn
Q:
Determine DrH for the following reaction,2 NH3(g) + 5/2 O2(g) 2 NO(g) + 3 H2O(g)given the thermochemical equations below.N2(g) + O2(g) 2 NO(g) DrH = +180.8 kJ/mol-rxnN2(g) + 3 H2(g) 2 NH3(g) DrH = -91.8 kJ/mol-rxn2 H2(g) + O2(g) 2 H2O(g) DrH = -483.6 kJ/mol-rxnA.-1178.2 kJ/mol-rxnB.-452.8 kJ/mol-rxnC.-394.6 kJ/mol-rxnD.-211.0 kJ/mol-rxnE.+1178.2 kJ/mol-rxn
Q:
Determine the enthalpy change for the decomposition of calcium carbonate
CaCO3(s) CaO(s) + CO2(g)
given the thermochemical equations below.
Ca(OH)2(s) CaO(s) + H2O() DrH = 65.2 kJ/mol-rxn
Ca(OH)2(s) + CO2(g) CaCO3(s) + H2O() DrH = -113.8 kJ/mol-rxn
C(s) + O2(g) CO2(g) DrH = -393.5 kJ/mol-rxn
2 Ca(s) + O2(g) 2 CaO(s) DrH = -1270.2 kJ/mol-rxn
A.+48.6 kJ/mol-rxn
B.+179.0 kJ/mol-rxn
C.+345.5 kJ/mol-rxn
D.+441.0 kJ/mol-rxn
E.+1711.7 kJ/mol-rxn
Q:
Determine the enthalpy change for the oxidation of ethanol to acetic acid,CH3CH2OH() + O2(g) CH3COOH() + H2O()given the thermochemical equations below.2 CH3CH2OH() + O2(g) 2 CH3CHO() + 2 H2O() DrH = -400.8 kJ/mol-rxn2 CH3CHO() + O2(g) 2 CH3COOH() DrH = -584.4 kJ/mol-rxnA.-985.2 kJ/mol-rxnB.-492.6 kJ/mol-rxnC.-183.6 kJ/mol-rxnD.+183.6 kJ/mol-rxnE.+492.6 kJ/mol-rxn
Q:
Determine the standard enthalpy of formation of Fe2O3(s) given the thermochemical equations below.Fe(s) + 3 H2O() Fe(OH)3(s) + 3/2 H2(g) DrH = +160.9 kJ/mol-rxnH2(g) + 1/2 O2(g) H2O() DrH = -285.8 kJ/mol-rxnFe2O3(s) + 3 H2O() 2 Fe(OH)3(s) DrH = +288.6 kJ/mol-rxnA.-252.6 kJ/mol-rxnB.+163.7 kJ/mol-rxnC.-824.2 kJ/mol-rxnD.+33.2 kJ/mol-rxnE.+ 890.6 kJ/mol-rxn
Q:
Determine the heat of evaporation of carbon disulfide,CS2() CS2(g)given the enthalpies of reaction below.C(s) + 2 S(s) CS2() DrH = +89.4 kJ/mol-rxnC(s) + 2 S(s) CS2(g) DrH = +116.7 kJ/mol-rxnA.-206.1 kJB.-27.3 kJC.+27.3 kJD.+206.1 kJE.+1.31 kJ
Q:
Acetylene, C2H2, is a gas used in welding. The molar enthalpy of combustion for acetylene is -2599 kJ. A mass of 0.338 g C2H2(g) is combusted in a bomb calorimeter. If the heat capacity of the calorimeter is 729 J/K and it contains 1.150 kg of water, what is the temperature increase of the bomb calorimeter? The specific heat capacity of water is 4.184 J/gK and the molar mass of acetylene is 26.04 g/mol.A.1.59 KB.6.09 KC.7.01 KD.12.3 KE.18.0 K
Q:
A 1.994 g sample of ethanol, CH3CH2OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 10.91 K. If the heat capacity of the bomb is 615.5 J/K and it contains 1.150 kg of water, what is the enthalpy change per mole of ethanol combusted? The specific heat capacity of water is 4.184 J/gK and the molar mass of ethanol is 46.07 g/mol.A.-5.921 101 kJ/molB.-2.563 103 kJ/molC.-1.181 105 kJ/molD.-1.368 103 kJ/molE.-122.7 103 kJ/mol
Q:
A chemical reaction in a bomb calorimeter evolves 3.86 kJ of energy in the form of heat. If the temperature of the bomb calorimeter increases by 4.17 K, what is the heat capacity of the calorimeter?
A.3.87 103 J/K
B.311 J/K
C.926 J/K
D.1.8 103 J/K
E.1.61 104 J/K
Q:
When 10.0 g KOH is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 25.18 C to 47.53 C. What is the enthalpy change per gram of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/gK.A.-116 J/gB.-934 J/gC.-1.03 103 J/gD.-2.19 103 J/gE.-1.03 104 J/g
Q:
Commercial cold packs consist of solid ammonium nitrate and water. NH4NO3 absorbs 25.69 kJ of heat per mole dissolved in water. In a coffee-cup calorimeter, 5.60 g NH4NO3 is dissolved in 100.0 g of water at 22.0 C. What is the final temperature of the solution? Assume that the solution has a specific heat capacity of 4.18 J/gK.A.0.0 CB.17.9 CC.11.6 CD.-54.8 CE.26.1 C
Q:
CaO(s) reacts with water to form Ca(OH)2(aq). If 6.50 g CaO is combined with 99.70 g H2O in a coffee cup calorimeter, the temperature of the resulting solution increases from 21.7 C to 43.1 C. Calculate the enthalpy change for the reaction per mole of CaO. Assume that the specific heat capacity of the solution is 4.18 J/gK.A.-1.45 kJ/molB.-82.0 kJ/molC.-9.42 kJ/molD.-165 kJ/molE.-532 kJ/mol
Q:
Hydrazine, N2H4, is a liquid used as a rocket fuel. It reacts with oxygen to yield nitrogen gas and water.N2H4() + O2(g) N2(g) + 2 H2O()The reaction of 6.50 g N2H4 evolves 126.2 kJ of heat. Calculate the enthalpy change per mole of hydrazine combusted.A.-19.4 kJ/molB.-25.6 kJ/molC.-126 kJ/molD.-622 kJ/molE.-820. kJ/mol
Q:
Iron oxide reacts with aluminum in an exothermic reaction.Fe2O3(s) + 2 Al(s) 2 Fe(s) + Al2O3(s)The reaction of 5.00 g Fe2O3 with excess Al(s) evolves 26.6 kJ of energy in the form of heat. Calculate the enthalpy change per mole of Fe2O3 reacted.A.-5.32 kJ/molB.-1.33 102 kJ/molC.-2.12 104 kJ/molD.-2.12 102 kJ/molE.-8.50 102 kJ/mol
Q:
The thermochemical equation for the combustion of butane is shown below.C4H10(g) + 13/2 O2(g) 4 CO2(g) + 5 H2O() DrH = -2877 kJ/mol-rxnWhat is the enthalpy change for the following reaction?8 CO2(g) + 10 H2O() 2 C4H10(g) + 13 O2(g)A.+1439 kJ/mol-rxnB.+2877 kJ/mol-rxnC.-5754 kJ/mol-rxnD.-2877 kJ/mol-rxnE.+5754 kJ/mol-rxn
Q:
The thermochemical equation for the combustion of methanol is shown below.CH3OH() + 3/2 O2(g) CO2(g) + 2 H2O(g) DrH = -638.7 kJ/mol-rxnWhat is the enthalpy change for the combustion of 8.59 g CH3OH?A.-171 kJB.-19.9 kJC.-2.38 103 kJD.-5.49 103 kJE.-1.76 106 kJ
Q:
Which of the following thermodynamic quantities are state functions: heat (q), work (w), enthalpy change (DH), and/or internal energy change (DU)?
A.q only
B.w only
C.DH only
D.DU only
E.DH and DU
Q:
Which of the following statements is/are CORRECT?
1/ If a reaction occurs at constant pressure, q = DH.
2/ The change in energy for a system is defined as the sum of the energies transferred as heat and work (i.e., DU = q + w).
3/ If a reaction occurs at constant volume, q = w
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
One statement of the first law of thermodynamics is that
A.the amount of work done on a system is dependent of the pathway.
B.the total work done on a system must equal the heat absorbed by the system.
C.the total work done on a system is equal in magnitude, but opposite in sign of the heat absorbed by the system.
D.the total energy change for a system is equal to the sum of the heat transferred to or from the system and the work done by or on the system.
E.in any chemical process the heat flow must equal the change in enthalpy.
Q:
The heat of vaporization of benzene, C6H6, is 30.7 kJ/mol at its boiling point of 80.1 C. How much energy in the form of heat is required to vaporize 102 g benzene at its boiling point?
A.0.302 kJ
B.23.6 kJ
C.24.2 kJ
D.40.1 kJ
E.3.14 103 kJ
Q:
What is the minimum mass of ice at 0.0 C that must be added to 1.00 kg of water to cool the water from 28.0 C to 12.0 C? (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/gK, liquid water = 4.184 J/gK)
A.175 g
B.201 g
C.244 g
D.299 g
E.1140 g
Q:
44.0 g of ice at -20.0 C is mixed with 325 g of water at 32.1 C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/gK, liquid water = 4.184 J/gK)A.-0.6 CB.5.5 CC.12.1 CD.17.6 CE.38.9 C
Q:
Calculate the energy in the form of heat (in kJ) required to change 75.0 g of liquid water at 27.0 C to ice at -20.0 C. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: ice = 2.06 J/gK, liquid water = 4.184 J/gK)A.-13.4 kJB.-17.7 kJC.-36.5 kJD.-10.2 kJE.-30.3 kJ
Q:
Calculate the energy in the form of heat (in kJ) required to convert 325 grams of liquid water at 20.0 C to steam at 115 C. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: liquid water = 4.184 J/gK, steam = 1.92 J/gK)
A.129 kJ
B.121 kJ
C.851 kJ
D.914 kJ
E.735 kJ
Q:
When 66.0 g of an unknown metal at 28.5 C is placed in 83.0 g H2O at 78.5 C, the water temperature decreases to 75.9 C. What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/gK.
A.0.055 J/gK
B.0.29 J/gK
C.0.69 J/gK
D.0.18 J/gK
E.2.6 J/gK
Q:
If 46.1 g Cu at 11.6 C is placed in 85.0 g H2O at 72.4 C, what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/gK and 4.184 J/gK, respectively.
A.71.2 C
B.63.6 C
C.51.0 C
D.42.0 C
E.69.5 C
Q:
If 35.0 g H2O at 22.7 C is combined with 65.0 g H2O at 87.5 C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/gK.
A.25.1 C
B.45.4 C
C.50.8 C
D.64.8 C
E.48.9 C
Q:
How much energy (in kJ) is required to change the temperature of 325 g aluminum from 32 C to 815 C? The specific heat capacity of aluminum is 0.897 J/gK.
A.238 kJ
B.284 kJ
C.46.3 kJ
D.228 kJ
E.2.16 kJ
Q:
If 50.0 g of benzene, C6H6, at 25.0 C absorbs 2.71 kJ of energy in the form of heat, what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/gK.
A.25.0 C
B.31.5 C
C.56.5 C
D.32.3 C
E.57.3 C
Q:
If the same amount of energy in the form of heat is added to 5.00 g samples of each of the metals below, which metal will undergo the largest temperature change?
Metal Specific Heat Capacity (J/gK)
Ag 0.235
Al 0.897
Cu 0.385
Fe 0.449
Hg 0.140
A.Ag
B.Al
C.Cu
D.Fe
E.Hg
Q:
If 495 J is required to change the temperature of 12.7 g of sodium chloride from 275.0 K to 335.0 K, what is the specific heat capacity of sodium chloride?
A.0.866 J/gK
B.2.60 J/gK
C.0.650 J/gK
D.1.15 J/gK
E.2.83 105 J/gK
Q:
Which of the following statements is/are CORRECT?
1/ Specific heat capacity is a positive value for liquids and solids and a negative value for gases.
2/ The larger the heat capacity of an object, the more thermal energy it can store.
3/ When heat is transferred from the surroundings to the system, q is negative.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Heat capacity is defined as
A.the amount of heat required to raise the temperature of 1 gram of substance by 1 K.
B.the amount of heat required to raise the temperature of a substance by 1 K.
C.the amount of heat required to vaporize a solid or liquid.
D.the maximum amount of heat that a substance may absorb without decomposing.
E.4.18 cal/gK.
Q:
Specific heat capacity is
A.the quantity of heat needed to change the temperature of 1.00 g of a substance by 1 K.
B.the quantity of heat needed to change the temperature of 1.00 g of a substance by 4.184 K.
C.the capacity of a substance to gain or lose a 1.00 J of energy in the form of heat.
D.the temperature change undergone when 1.00 g of a substance absorbs 4.184 J.
E.the maximum amount of energy in the form of heat that 1.00 g of a substance may absorb without decomposing.
Q:
Which of the following processes is/are exothermic?
1/ the reaction of butane with oxygen
2/ the melting of gold
3/ cooling copper from 225 C to 65 C
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
Q:
Which of the following processes is/are endothermic?
1/ the combustion of hydrogen
2/ the condensation of water
3/ the evaporation of isopropyl alcohol
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
Q:
Many homes are heated using natural gas. The combustion of natural gas converts
A.chemical potential energy to thermal energy.
B.thermal energy to mechanical energy.
C.mechanical energy to chemical potential.
D.electrostatic energy to mechanical energy.
E.gravitational energy to acoustic energy.
Q:
Which one of the following statements is INCORRECT?
A.Energy is neither created nor destroyed in chemical reactions.
B.Kinetic energy is the energy that results from an object's position.
C.Exothermic processes transfer heat from the system into the surroundings.
D.Increasing the thermal energy of a gas increases the motion of its atoms.
E.Energy is the capacity to do work.
Q:
A hot piece of iron is dropped into a beaker containing colder water. Which of the following statements is/are CORRECT?
1/ Energy is transferred as heat from the iron to the water.
2/. Thermal equilibrium is attained when the iron and the water reach the same temperature.
3/ Thermal energy from the iron is converted to electrostatic energy in the water.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Which of the following statements is/are CORRECT?
1/ A system is defined as an object or collection of objects being studied.
2/ Surroundings are defined as the entire universe, including the system.
3/ In an endothermic reaction, heat is transferred from the system to the surroundings.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
Q:
In combustion analysis, the gases produced by the combustion of a hydrocarbon are passed through a tube containing finely divided NaOH supported on asbestos. The purpose of the NaOH is to absorb ________ produced by the combustion reaction.
Q:
The reaction of 5.07 g N2 with 0.722 g H2 produces 1.27 g NH3. The percent yield of this reaction is ________.
Q:
PCl3 can be produced from the reaction of P4 with Cl2.
P4(s) + 6 Cl2(g) 4 PCl3(g)
If 1.00 g P4 reacts with 1.00 g Cl2, which reactant is the limiting reactant? What mass of product may be produced?
Q:
The following equation: A = e C (where is path length and C is concentration) is known as the _____-Lambert law.
Q:
The pH of purified water (or of a neutral solution) is _____.
Q:
The percent yield of a chemical reaction is calculated by dividing the actual yield by the ________ yield and multiplying by 100%.
Q:
The numbers preceding the formulas in chemical equations are referred to as the ________ coefficients.
Q:
Which of the following statements is/are CORRECT?
1/ Absorbance is directly proportional to the intensity of the incident light.
2/ Absorbance is inversely proportional to the analyte concentration.
3/ Absorbance is directly proportional to the path length of the light.
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1,2, and 3
Q:
Transmittance, T, is defined as the intensity of light transmitted through a sample divided by the intensity of light incident on the sample. The absorbance, A, is defined asA.A = -log TB.A = log (-T)C.A = 10TD.A = 10-TE.A = 10-1/T
Q:
If 0.1800 g of impure soda ash (Na2CO3) is titrated with 15.66 mL of 0.1082 M HCl, what is the percent purity of the soda ash?
Na2CO3(aq) + 2 HCl(aq) 2 NaCl(aq) + H2O() + CO2(g)
A.17.96%
B.49.89%
C.50.11%
D.94.13%
E.99.77%
Q:
A 25.00 mL sample of NaOH is titrated with 26.14 mL of 0.1750 M HCl(aq). What is the concentration of the NaOH solution?
A.1.995 10-4 M
B.0.09149 M
C.0.1830 M
D.0.1674 M
E.0.08945 M
Q:
A mass of 0.4113 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 28.10 mL of 0.1055 M NaOH(aq), what is the molar mass of the acid?A.2.965 10-3 g/molB.9.128 g/molC.138.7 g/molD.337.3 g/molE.820.7 g/mol
Q:
What volume of 0.250 M KCl(aq) will completely react with 50.0 mL of 0.115 M Pb(NO3)2(aq)?
2 KCl(aq) + Pb(NO3)2(aq) PbSO4(s) + 2 KNO3(aq)
A.23.0 mL
B.46.0 mL
C.11.5 mL
D.109 mL
E.218 mL
Q:
Zn reacts with hydrochloric acid.
Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g)
What volume of 3.05 M HCl(aq) will react with 25.0 g Zn(s)?
A.0.251 L
B.4.01 L
C.0.125 L
D.0.0627 L
E.2.33 L
Q:
An aqueous nitric acid solution has a pH of 2.15. What mass of HNO3 is present in 20.0 L of this solution?
A.0.11 g
B.0.022 g
C.3.7 g
D.6.8 g
E.8.9 g
Q:
The pH of a vinegar solution is 4.15. What is the H3O+ concentration of the solution?A.7.1 10-5 MB.1.6 10-2 MC.0.62 MD.1.4 ME.1.4 104 M
Q:
The pH of an aqueous NaOH solution is 12.83. What is the hydrogen ion concentration of this solution?A.1.5 10-13 MB.6.7 10-2 MC.1.2 MD.6.7 1012 ME.2.7 10-6 M
Q:
What is the pH of 3.5 10-3 M HCl(aq)?A.-1.01B.2.46C.3.50D.1.01E.5.65
Q:
What volume of 3.0 M HNO3(aq) must be diluted to make 4.0 L of 0.20 M HNO3(aq)?
A.6.0 L
B.0.15 L
C.0.20 L
D.0.27 L
E.2.4 L
Q:
If 25.00 mL of 1.50 M HCl(aq) is diluted with water to a volume of 750.0 mL, what is the molarity of the diluted HCl(aq)?
A.2.22 10-2 M
B.5.00 10-2 M
C.2.07 10-3 M
D.4.50 101 M
E.1.35 103 M
Q:
What is the mass of potassium iodide in 50.0 mL of 5.75 10-2 M KI(aq)?A.2.88 10-2 gB.191 10-1 gC.6.92 10-3 gD.4.77 10-1 gE.191 102 g
Q:
If 5.15 g Fe(NO3)3 is dissolved in enough water to make exactly 150.0 mL of solution, what is the molar concentration of nitrate ion?
A.0.00319 M
B.0.0343 M
C.0.142 M
D.0.313 M
E.0.426 M
Q:
How many liters of 0.1107 M KCl(aq) contain 2.50 g of KCl?
A.0.277 L
B.0.303 L
C.3.71 10-3 L
D.3.30 L
E.5.94 10-4 L
Q:
If 4.49 g NaNO3 is dissolved in enough water to make 250.0 mL of solution, what is the molarity of the sodium nitrate solution?A.1.80 10-2 MB.5.28 10-2 MC.2.11 10-1 MD.1.32 10-2 ME.18.0 M
Q:
Naphthalene, a hydrocarbon, has an approximate molar mass of 128 g/mole. If the combustion of 0.6400 g naphthalene produces 0.3599 g H2O and 2.1977 g CO2, what is the molecular formula of this compound?
A.C8H32
B.C9H18
C.C9H20
D.C10H8
E.C11H7
Q:
An unknown hydrocarbon contains carbon, hydrogen, and oxygen. Combustion of 1.5000 g of the hydrocarbon produces 1.1738 g H2O and 2.1505 g CO2. What is the empirical formula of the hydrocarbon?
A.CHO
B.C2H3O
C.C3H4O
D.C3H8O3
E.C5H5O
Q:
Soft drink bottles are made of polyethylene terephthalate (PET), a polymer composed of carbon, hydrogen, and oxygen. If 1.9022 g PET is burned in oxygen it produces 0.6585 g H2O and 4.0216 g CO2. What is the empirical formula of PET?
A.CHO
B.CH7O5
C.C5H7O
D.C8H10O
E.C10H8O5