TIGER

Assessment Questions: 43 results
Thermodynamics : ConservGibbsEnergy (6 Variations)
Which of the following best illustrates conservation of Gibbs free energy?
Thermodynamics
Equilibrium : CalcRxnQuotient (13 Variations)
In an experiment, 4.44 mol of SO2, 7.93 mol of O2 and 4.03 mol of SO3 are placed in a 2.0L reaction vessel at a certain temperature. Calculate the reaction quotient, Q, for the reaction as written:

What is the calculated reaction quotient, Q? {2:NUMERICAL:=2.1e-1:1e-2#Correct! ~%50%2.1e-1:5e-2#Close but not quite right}

If Kc for this reaction at the temperature of the experiment is 3.7 x 103, will the reaction move toward the left or toward the right? {1:MULTICHOICE:left#Sorry, that's wrong.~=right#Correct!}


Equilibrium |
Chemometrics
Thermodynamics : InterpretKandDeltaG (16 Variations)
The thermodynamic equilibrium constant for the following reaction is 0.15 at 1227°C.
2 SO2(g) + O2(g) 2 SO3(g)
Check the box for each true statement.

Thermodynamics
Thermodynamics : CalcDeltaG (14 Variations)
Using , calculate the Gibbs free energy change for the following reaction which produces the metal zinc from its ore zinc(II) oxide.
2 ZnO(s) 2 Zn(s) + O2(g)


Thermodynamics |
Chemometrics
Thermodynamics : ATPFromGlucose (8 Variations)
When glucose is oxidized in the human body it releases a lot of Gibbs free energy. Rather than waste this free energy, the body stores much of it in the form of ATP. The following reaction shows this process of storing some of the energy from glucose in ATP. This is an example of coupled reactions in a biological system.

The label on a can of Coke says that it contains 39 g of sugar. Assume that all of the sugar is glucose (even though it isn't), and calculate how many moles of ATP can be produced theoretically by the oxidation of 39.0 g of glucose.

Thermodynamics |
Reactions |
Chemometrics
Thermodynamics : GibbsFromHSandT (5 Variations)
On the space shuttle, the carbon dioxide produced by the astronauts is handled by an environmental control system that utilizes the following reaction.

H° = -138.4 kJ and S° = -139 J/K Calculate G° at 25°C for this reaction.

Thermodynamics |
Chemometrics
Equilibrium : EquilTrueFalse (4 Variations)
Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium?
Equilibrium
Equilibrium : KspExpressions (10 Variations)
What is the solubility product expression for Ag3PO4?
Equilibrium
Equilibrium : KspSaturation (12 Variations)
Zn(OH)2 has a Ksp of 4.5 x 10-17. If you have a solution of Zn(OH)2 that has a hydroxide ion concentration equal to 4.6 x 10-6 mol/L, the solution is ... (Assume that the only relevant reaction is the solubility-product equilibrium.)
Equilibrium
Equilibrium : LeChatPrinciple (18 Variations)
Consider the following equilibrium, established in a 2 L flask at 30oC.

CO(g) + H2O(g) CO2(g) + H2(g) H0= -41.2 kJ

What will happen to the concentration of CO2 if the temperature is increased?


Equilibrium
Equilibrium : RxnDirectAndTemp (16 Variations)
2 SO2(g) + O2(g) 2 SO3(g)
The reaction above has an equilibrium constant of 0.25 at 830oC, and Horxn = -197.78 kJ/mol under standard conditions. Under which conditions will this reaction produce the most sulfur trioxide?

Equilibrium
Equilibrium : EquilExpressions (15 Variations)
What is the correct equilibrium constant expression for the balanced reaction shown below?

C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l)


Equilibrium
Equilibrium : InterpretEqConsts (12 Variations)
The following reaction has an equilibrium constant of 1.2x1018 at 25oC.

CH4(g) + Cl2(g) CH3Cl(g) + HCl(g)

Which of the following statements is true?


Equilibrium
Equilibrium : ICETables (16 Variations)
2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)

You have 0.4 moles C2H2 and 0.2 moles O2 present initially in a 5L flask. You allow the reaction to run until it reaches equilibrium. Which of the following is the correct ICE table for this process?


Equilibrium
Equilibrium : SolubilityPressTemp (16 Variations)
How does increasing the temperature change the solubility of nitrogen in water?
Equilibrium
Thermodynamics : CompareEntropyQual (16 Variations)
Indicate which substance in each of the following pairs of substances you expect to have higher entropy. Assume that you have a mole of each substance and all substances are at the same temperature.
Thermodynamics
Thermodynamics : PredictEntropyChange (10 Variations)
For each of the following processes, indicate whether you expect the entropy change of the system to be positive or negative.
Thermodynamics
Thermodynamics : GeneralThermo (6 Variations)
Which of the following statements is an inaccurate statement about thermodynamics?
Thermodynamics
Thermodynamics : ProbabilityEnergyDist (23 Variations)
Consider a system that has two indistinguishable molecules that can occupy three different energy levels (having energies of 1kJ, 2kJ and 3kJ, respectively). What is the probability that the molecules will have a total energy of 2 kJ?
Thermodynamics
Thermodynamics : ThermoKinStability (4 Variations)
Compare white and grey tin, both of which exist as solid phases of tin near room temperature.

Phase Hof (kJ/mol) So (J/(K*mol))
white tin 0 51.5
grey tin -2.1 44.8

Which type of stability does each exhibit at 40 oC?

white tin {1:MULTICHOICE:kinetically stable#No, that's incorrect.~=thermodynamically stable#Correct!}

grey tin {1:MULTICHOICE:=kinetically stable#Correct!~thermodynamically stable#No, that's incorrect.}


Thermodynamics
Equilibrium : CommonIonEffect (9 Variations)
The molar solubility of lead(II) fluoride (PbF2) is 2.1 x 10-3 mol/L in pure water at 25oC. What is the molar solubility of lead(II) fluoride in 0.10 M NaF at 25oC? (Assume that the only relevant reaction is the solubility-product equilibrium.)
Equilibrium |
Chemometrics
Equilibrium : ConcFromKsp (8 Variations)
The Ksp of BaF2 is 1.7 x 10-6 mol/L in water at 25oC. What is the concentration of barium ions in equilibrium with solid barium fluoride? (Assume that the only relevant reaction is the solubility-product equilibrium.)
Equilibrium |
Chemometrics
Equilibrium : InterpretKsp (16 Variations)
Which of the following salts would give you the highest concentration of phosphate ions in solution if you placed 1 mole of the salt in a liter of water?
Equilibrium |
Chemometrics
Equilibrium : EquilAndRxnRates (8 Variations)

For the reaction of A B, which of the following statements about the rates of forward and reverse reactions is true at time x?

Equilibrium |
Kinetics
Equilibrium : EqConstRelationships (12 Variations)
The equilibrium constant for the reaction of hydrogen gas and ethene to produce ethane under certain conditions is 9.8 x 1018.
H2(g) + C2H4(g) C2H6(g) K = 9.8 x 1018

What is the equilibrium constant for the following reaction under the same conditions?
C2H6(g) H2(g) + C2H4(g) K = ?


Equilibrium |
Chemometrics
Equilibrium : CalcMolesAtEquil (15 Variations)
The following reaction has an equilibrium constant of 0.083 at 900oC.

COCl2(g) CO(g) + Cl2(g)

If you have 1.00 mole of COCl2(g) in a 1.00L container initially, how many moles of COCl2 will be present when the system reaches equilibrium?


Equilibrium |
Chemometrics
Equilibrium : EqConstConcData (4 Variations)
SbCl5(g) SbCl3(g) + Cl2(g)

You have 0.50 mol SbCl5 present initially in a 1.0L flask. The system is allowed to reach equilibrium at 450oC. There is 0.10 mol Cl2 present at equilibrium. What is the equilibrium constant, K?


Equilibrium |
Chemometrics
Equilibrium : CalcKp (2 Variations)
In one experiment chemists studied the formation of phosgene, COCl2, by mixing {y} atm of carbon monoxide and {z} atm of Cl2 in a reaction vessel at 700K. After the system reached equilibrium, the total pressure was {x} atm. Calculate Kp for the reaction.

Hint: Remember that the total pressure is the sum of all the partial pressures.

Note:
      Do Not use scientific notation
      DO NOT use spaces
      DO NOT write in the units.
      Be sure to write your answer with only one decimal place even if this is not the correct number of significant figures.

Equilibrium |
Chemometrics
Equilibrium : CalcKc (4 Variations)
A container initially has {y} M ammonia at a certain temperature. When the system reaches equilibrium the concentration of ammonia is {x} M. Calculate Kc for the following reaction as written.

Note:
      Answers must be written using scientific notation with "e"
      DO NOT use spaces
      DO NOT write in the units.
      Be sure to use three significant figures.
          eg:       2.44e-5

Equilibrium |
Chemometrics
Equilibrium : ConvertKcKp (6 Variations)
Nitrosyl bromide is formed from nitrogen oxide and bromine:

Kp for this reaction is {x} at {y}°C. Calculate Kc at this temperature. (R = 0.0821 L atm/mol K)

Note:
DO NOT use scientific notation
Use integers (no decimal places) even is this is not the correct number of significant figures.
DO NOT write in the units.
eg: 18


Equilibrium |
Chemometrics
Equilibrium : MoreMolesAtEquil (19 Variations)
The following reaction has an equilibrium constant of 0.050 at a given temperature.

N2(g)+ O2(g) 2NO(g)

If you have 0.75 moles of N2(g) and 0.75 moles of O2(g) in a 2.0L container initially, how many moles of N2 will be present when the system reaches equilibrium?


Equilibrium |
Chemometrics
Thermodynamics : CalcDeltaS (9 Variations)
Using , calculate the entropy change for the reaction.

Thermodynamics |
Chemometrics
Thermodynamics : CalcMinSpontTemp (9 Variations)
Calculate the minimum temperature above which the following reaction will be product-favored (spontaneous).



Thermodynamics |
Chemometrics
Thermodynamics : DetermineRxnFavored (8 Variations)
When industrial plants burn coal, sulfur dioxide is produced. Sulfur dioxide is a primary pollutant that contributes to both industrial smog and acid rain. Is this process of producing sulfur dioxide product-favored?

Using


Thermodynamics |
Chemometrics
Acids_and_Bases : PercentDissociationKa (3 Variations)
Calculate the percent dissociation in a {x}M aqueous solution of the weak acid HA. (Ka = {y} x 10-4)

Enter your answer to ONE decimal place.
DO NOT use scientic notation.
DO NOT write in the units.


Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
Equilibrium
Thermodynamics : EntropyPhaseChange (13 Variations)
Aluminum can be evaporated in a vacuum to form highly reflective coatings. Aluminum boils at 2792K and has a heat of vaporization of 70.0 kcal/mol. Calculate the entropy change for the vaporization of one mole of aluminum.
Thermodynamics |
Chemometrics |
Phases / Phase Transitions / Diagrams
Acids_and_Bases : WeakAcidSolnpH (20 Variations)
Given an aqueous solution of 0.30 M acetic acid (Ka = 1.8 x 10-5), the pH is approximately ...
Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium
Acids_and_Bases : BufferingCapacity (20 Variations)
If a buffer is prepared using 0.75 mol CH3COOH and 0.45 mol CH3COO- in 1 liter of aqueous solution, is the buffering capacity of the solution great enough to maintain its pH if 10 g NaOH is added?
Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium
Acids_and_Bases : pHDilution (6 Variations)
What is the pH of a solution made by diluting {x} mL of {y} M HNO3(aq) to a total volume of 500 mL?

Enter your answer to two decimal places.
DO NOT use scientific notation

Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium
Acids_and_Bases : pHBufferCalc (4 Variations)
Calculate the pH of a buffer solution containing {x}M NH3 and {y}M NH4NO3.

Enter your answer to TWO decimal places.
DO NOT use scientific notation.
DO NOT enter units
        eg:     4.55

Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium
Acids_and_Bases : BufferWeakStrong (7 Variations)
How many mL of a 2.50 M HCl solution must be added to 500 mL of a 0.150 M CO32- solution to make a buffer with pH = 10.00?
Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium
Acids_and_Bases : CalcSolnpH (5 Variations)
Use this acid/base table to answer the question below.

Calculate the pH of a {x}M sodium acetate solution.

DO NOT use scientific notation
Enter your answer to two decimal places.
DO NOT enter units

Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium
Acids_and_Bases : BufferWeakWeak (14 Variations)
What mass of potassium bicarbonate (KHCO3) must be added to 500 mL of a 0.200 M carbonic acid solution to make a buffer with pH = 6.30?
Acids / Bases |
Reactions |
Aqueous Solution Chemistry |
pH |
Equilibrium