TIGER

Assessment Questions: 40 results
Solutions : FreezePtDepression (20 Variations)
It takes 6.86 kg of ethylene glycol (antifreeze) to decrease the freezing point of 6.50 kg of water to -25.0oF (-31.7oC). How much sodium chloride (NaCl) would it take to decrease the freezing point of 6.50 kg of water to -25.0oF? (Assuming all the salt will dissolve in that amount of water.)
Solutions / Solvents
Solutions : GeneralSolutions (10 Variations)
You have 500.0mL of 0.100M aqueous MgBr2. Which of the following statements are true?
Solutions / Solvents
Solutions : SolnPrepProcedure (10 Variations)
You want to prepare 250mL of a 0.0150M solution of KCl. Which of the following procedures would give you the best results?
Solutions / Solvents
Solutions : SolutionNanoPics (4 Variations)
The drawings below represent flasks of aqueous solutions. Each pink dot represents a dissolved solute particle.
Which of the following solutions is most concentrated?

500 mL
Solution A
500 mL
Solution B
500 mL
Solution C
250 mL
Solution D
250 mL
Solution E
250 mL
Solution F


Solutions / Solvents
Thermochemistry : SystemSurrExoEndo (4 Variations)
Sulfuric acid is added to water in a beaker and the resulting solution is much warmer than either the water or acid was initially.
Identify the following items as being part of the system or the surroundings, and indicate whether the process is exothermic or endothermic.

Calorimetry / Thermochemistry
Thermochemistry : BondEnergies (10 Variations)
Use to determine which of the following requires the most energy.
Calorimetry / Thermochemistry
Thermochemistry : FlaskTemp (6 Variations)
If 200. J of thermal energy was added to both flasks, which of the following would happen?

Calorimetry / Thermochemistry
Thermochemistry : GeneralEnergy (10 Variations)
Which of the following statements about energy is NOT true?
Calorimetry / Thermochemistry
Thermochemistry : ThermalEnergy (2 Variations)
The sketch below shows two identical flasks with different volumes of water at the same temperature. Which of the following is true?

Calorimetry / Thermochemistry
Thermochemistry : HeatTransfers (10 Variations)
A red-hot piece of lead is dropped into water. Which of the following statements are true? (Assume that there are no energy transfers between anything except the lead and the water.)
Calorimetry / Thermochemistry
Solutions : IonConcentration (4 Variations)
Which of the following solutions has the greatest concentration of Na+ ions?
Solutions / Solvents |
Chemometrics
Solutions : MassSoluteInSoln (10 Variations)
What is the mass of the solute in 500mL of 0.341M ammonium chloride?
Solutions / Solvents |
Chemometrics
Solutions : RelativeConc (4 Variations)
What are the relative concentrations of the ions in 0.10 M aqueous sulfuric acid?
Solutions / Solvents |
Stoichiometry
Solutions : ReverseOsmosis (20 Variations)
You are given a water sample that contains ammonium chloride (NH4Cl). You determine the concentration of the salt to be 0.500 M and decide to purify the water using reverse osmosis. What is the minimum pressure that must be applied at 30.0oC to force the water through the membrane?
Solutions / Solvents |
Transport Properties
Solutions : SolnConcAfterMixing (4 Variations)
10 mL of 0.1 M BaCl2(aq) is mixed with 10 mL of 0.1 M AgNO3(aq). What are the concentrations of the ions in the final mixture?
Solutions / Solvents |
Chemometrics
Solutions : SolnPrepByDilution (10 Variations)
For the analysis of trace metals it is necessary to prepare solutions of very low concentrations from a stock solution of higher concentration using a micropipet and a volumetric flask. What volume of a 0.0010 M solution of Zn(NO3)2 (aq) would be required to prepare a 5.0 nM solution of Zn2+ in a 250mL flask?
Solutions / Solvents |
Chemometrics
Solutions : SolnPrepByMass (4 Variations)
You are required to prepare 5 L of a solution containing 1.000 x 10-3 mol/L of Cu2+(aq). Which of the following procedures would produce an appropriate solution?
Solutions / Solvents |
Chemometrics
Thermochemistry : BombCalorimeter (4 Variations)
Stearic acid (CH3(CH2)16CO2H) is a fatty acid, the part of fat that stores most of the energy. 1.00 g of stearic acid was burned in a bomb calorimeter. The bomb had a heat capacity of 652 J/oC and a 500. g water reservoir. If the temperature rose from 25.0 to 39.3 oC, how much heat was released when the stearic acid was burned?
Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : CalcHStateChange (4 Variations)
Calculate the enthalpy change when 100. g of ice at 0.0 oC is heated to liquid water at 50.0oC. (The heat of fusion for water is 333 J/g.)
Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : CoffeeCupCalorimeter (2 Variations)
A block of copper is heated to {x} °C and then is dropped into a coffee cup calorimeter containing {y} g of water at 25.0 °C. The final temperature of the system is 45.1 °C. What is the mass of the copper block to the nearest gram? (Assume all heat is transferred to the water). Write your answer in the box, and do NOT include units.

Specific heat capacity of copper = 0.383 J/(g*°C)

Specific heat capacity of water = 4.18 J/(g*°C)

Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : FuelAmpWattHeat (4 Variations)
Gasoline has an enthalpy of combustion of approximately 24000 kJ/gallon. When gasoline burns in an automobile engine, approximately 30% of the energy released is used to produce mechanical work. The remainder is lost as heat transfer to the engine's cooling system and eventually the atmosphere. As a start on estimating how much heat transfer is required, calculate what mass of water could be heated from 25 to 100oC by the combustion of 1.0 gallon of gasoline in an automobile.
Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : HeatCapacityGraph (6 Variations)

Consider the graph above. Which of these substances has the highest specific heat capacity?


Calorimetry / Thermochemistry |
Heat Capacity
Thermochemistry : HeatCapacityLiq (4 Variations)
100 g of water (c=4.184 J/g.oC), 100 g of ethanol (c=2.46 J/g.oC), 100 g of carbon tetrachloride (c=0.861 J/g.oC), and 100 g of ethylene glycol (c=2.42 J/g.oC) at 50oC were each placed into a separate coffee cup calorimeter and the temperature recorded. The temperature of the surroundings was 20oC. After one hour the temperature of which substance would have changed by the largest amount? Assume that the rate of heat transfer from the coffee cup to the surroundings was the same in each case.
Calorimetry / Thermochemistry |
Heat Capacity
Thermochemistry : CalcHBondEnergy (14 Variations)
Use the bond energies given in to estimate the Ho for the reaction given below:

hint: both carbon dioxide and molecular oxygen have double bonds


Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : CalcHCombustion (6 Variations)
Using the thermodynamic data given in , determine the enthalpy change for the combustion of ethane to produce carbon dioxide and water vapor.

2C2H6(g) + 7O2(g) 4CO2(g) + 6 H2O(g)


Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : EnthalpyEnergy (10 Variations)
2SO2(g) + O2(g)2SO3(g)
Horxn = -197.78 kJ
How much energy is transferred when 96.6 g of SO2 reacts to form SO3?

Calorimetry / Thermochemistry |
Chemometrics
Bonding : EnergyBreakAllBonds (10 Variations)
Use the bond energies given in to determine the total energy needed to break all of the bonds in C3H6. (Do not use ring structures.)
Covalent Bonding |
Calorimetry / Thermochemistry
Thermochemistry : HeatCapacitySolLiq (4 Variations)
The Table below lists the specific heat capacities of several metals and liquids.

Substance Specific Heat Capacity
J/(g.oC)
Substance Specific Heat Capacity
J/(g.oC)
Al 0.902 H2O 4.18
Fe 0.451 C2H5OH 2.46
Cu 0.383 CCl4 0.861
Au 0.128 CCl2F2 0.598

In an experiment, 50 g of a metal was heated to 100oC and placed in 200 g of a liquid at 25oC. Which of the following combinations of metal and liquid will produce the largest temperature increase in the liquid? (Assume that there is no transfer of energy to the surroundings.)


Calorimetry / Thermochemistry |
Heat Capacity
Thermochemistry : CalcHHessLaw (8 Variations)
The industrial process for making sulfuric acid has three steps. Using the data given, calculate the enthalpy change for the overall reaction for the process (the equation is given below).

2S(s) + 3O2(g) + 2H2O(l)2H2SO4(l)

Data:

S(s) + O2(g) SO2(g) Hrxn = -296.83 kJ
2SO3(g)O2(g) + 2SO2(g) Hrxn = -198.2 kJ
SO3(g) + H2O(l)H2SO4(l) Hrxn = -227.72 kJ


Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : MassFromCalorimetry (2 Variations)
The table below lists the specific heat capacities of several metals and liquids.

SubstanceSpecific Heat Capacity
J/(g.oC)
SubstanceSpecific Heat Capacity
J/(g.oC)
Al0.902H2O4.18
Fe0.451C2H5 OH2.46
Cu0.383CCl40.861
Au0.128CCl2F2 0.598

In an experiment a block of aluminum was heated to 100oC and placed in 200 g of water at 25oC. If the final temperature of the system is 43oC, and no heat transfer to the surroundings occurred, what is the mass of the aluminum block?


Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : CalcMolarEnthalpy (5 Variations)
White phosphorus, P4, ignites in air to produce heat, light, and P4O10 according to the following reaction.

P4(s) + 5O2(g) P4O10(s)

If 67.2 g of P4 is burned,1620 kJ of energy is evolved. What is the molar enthalpy of combustion of P4 if the process was carried out under constant pressure?


Calorimetry / Thermochemistry |
Chemometrics
Thermochemistry : ConvertEnergyUnits (4 Variations)
The label on a granola bar says it provides 120 Calories. How many kilojoules of energy will this bar provide if it is completely metabolized?
Calorimetry / Thermochemistry |
Nomenclature / Units / Symbols
Solutions : ConvertConcUnits (10 Variations)
The maximum concentration of arsenic in drinking water that is allowed by the EPA is 0.050 mg/L. Express this as a weight percent. (You can assume the density of the water solution is 1.0g/mL.)
Solutions / Solvents |
Nomenclature / Units / Symbols |
Chemometrics
Solutions : GramsToMolalSoln (20 Variations)
How many grams of citric acid need to be added to 750 ml of ethanol to make a 0.50 m solution?

Density (g/ml)

Molecular Weight (g/mol)

Citric acid

1.665

192.14

Ethanol

0.7893

46.07


Solutions / Solvents |
Nomenclature / Units / Symbols |
Chemometrics
Solutions : MixturesMolcPics (11 Variations)
Which of the following combinations of substances corresponds to the molecular scale diagram shown below?

Solutions / Solvents |
Noncovalent Interactions |
Precipitation / Solubility
Solutions : WtPercentToMolarity (4 Variations)
A common concentration unit used commercially is percent weight per volume (%W/V) which is the number of grams of solute in 100 mL of solution. A bottle of vinegar contains 5 %W/V acetic acid (CH3COOH). What is the molar concentration of acetic acid in the vinegar?
Solutions / Solvents |
Nomenclature / Units / Symbols |
Chemometrics
Solutions : CalcMolarityFromPPT (10 Variations)
You are given a water sample to analyze from a lake contaminated with lead. It takes 24 mL of 0.020 M NaCl to exactly precipitate the Pb2+ ions from 61 mL of the water sample. What is the concentration of Pb2+ ions in the water?
Pb2+(aq) + 2NaCl(aq)PbCl2(s) + 2Na+(aq)

Solutions / Solvents |
Nomenclature / Units / Symbols |
Chemometrics
Thermochemistry : PhaseChangeEnthalpy (10 Variations)
A solid melts to a liquid. Which of the following statements are true? (Assume constant pressure and a flexible container.)
Calorimetry / Thermochemistry |
Phases / Phase Transitions / Diagrams
Thermochemistry : PhaseChanges (8 Variations)
Steam at 100oC is condensed by an ice-water mixture at 0oC. Assuming that there is still ice present when the process is over, how much ice will be melted if 10.0 g of steam is condensed? The following may be useful:
enthalpy of vaporization of water = 40.7 kJ/mol; enthalpy of fusion of water = 6.07 kJ/mol; specific heat capacity of water = 4.184 J/g•K.

Calorimetry / Thermochemistry |
Phases / Phase Transitions / Diagrams
Intermolecular_Forces__Liquids_and_Solids : PhaseEnergyChanges (6 Variations)
When a liquid is transformed into its vapor at constant temperature,
Phases / Phase Transitions / Diagrams |
Calorimetry / Thermochemistry