Chem 104 Final Practice Problems
Draw out 2-bromo-4-isopropylheptane
(Toolbox 2 GHW problem 4)
Choose the oxidation state for the metal found in Fe2O3.
+3
Rank the following acids in order of weakest to strongest acid.
- 1 (weakest) H2O - 2 HCN - 3 HOCl - 4 (strongest) HClO4
Consider the titration of 50.0 mL of 1.00 M C5H5N by 0.500 M HCl. For each volume of HCl added, decide which of the components is a major species after the HCl has reacted completely. Kb for C5H5N = 1.7 x 10-9. -0.00 mL HCl added -30.00 mL HCl added -100.00 ml HCl added -150.00 mL HCl added -Calculate the pH at the equivalence point for this titration. -At what volume of HCl added in this titration does the pH = 5.23?
- C5H5N + H2O -H2O + Cl- + C5H5N + C5H5NH+ -H2O + Cl- + C5H5NH+ -H2O + Cl- + C5H5NH+ -2.85 -50mL
Consider the titration of 40.0 mL of 0.400 M HI by 0.300 M NaOH. -Calculate the pH after 37.7 mL of NaOH has been added. -At what volume (in mL) of NaOH added does the pH of the resulting solution equal 7.00? Include the units of mL in your answer.
-1.22 -53.3mL
The next three (3) problems deal with the titration of 351 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.1 M KOH. -What is the pH of the solution at the 2nd equivalence point? -What will the pH of the solution be when 0.2894 L of 1.1 M KOH are added to the 351 mL of 0.501 M carbonic acid? -How many mL of the 1.1 M KOH are needed to raise the pH of the carbonic acid solution to a pH of 6.844?
-11.84 -10.88 -119.9
N2(g) + 3H2(g) → 2NH3(g) This is the Free Energy measured under standard conditions, when the reaction is started with 1.0 M of each of the three gases present. Calculate the non-standard Free Energy change (∆G) at 298 K, given the following non-standard initial concentrations of the three gases. Answer in kJ. ∆Gf = -16.6 kJ/mol for NH3 (g) at 298 K -N2 = 1.0M -H2 = 0.1M -NH3 = 2.2M
-12.18 kJ
What is the maximum amount of work (in kJ) that could be supplied by the following reaction under the given conditions at 319 K? C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (g) where ΔHrxn = -1323 kJ, ΔSrxn = -28.1 J/K, and [C2H4] = 4.07 M, [O2] = 14.51 M, [CO2] = 8.69 M, and [H2O] = 14.57 M.
-1310kJ
1.00 L of 2.00 M HBr is titrated with 3.00 M KOH. -How many moles of acid are equal to one equivalent in this titration? -How many moles of HBr are found in solution at the halfway point of the titration? -How many liters of base will be needed to reach the equivalence point of the titration?
-2 moles -1 mole -0.6666 L
consider 1.0 L of a solution which is 0.55 M HF and 0.2 M NaF -Calculate the pH of this solution. -Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on addition of HCl. -Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH
-2.7 -2.33 -3.20
Consider the titration of 50.0 mL of 0.200 M HOCl by 0.200 M KOH for the next five questions (Ka for HOCl = 3.5 x 10-8). -Calculate the pH after 0.0 mL of KOH has been added. -Calculate the pH after 10.0 mL of KOH has been added. -Calculate the pH after 25.0 mL of KOH has been added. -Calculate the pH at the equivalence point. -Calculate the pH after 150.0 mL of KOH has been added.
-4.1 -6.85 -7.46 -10.23 -13
Consider a the titration of 1.0 M ascorbic acid (H2C6H6O6, Ka1 = 7.9e-5, Ka2 = 1.6e-12) with 2.0 M NaOH. -What is the pH at the first halfway point of the titration? - pH at the second halfway point of the titration? - pH at the equivalence point?
-4.102 -11.795 -7.948
Calculate the free energy change at 30 degrees C for the reaction shown: 2 NO2 (g) → N2O4 (g) ∆Hrxn = -58.04 kJ ∆Srxn = -176.9 J/K
-4.41 kJ
Consider the titration of 100.0 mL of 0.39 M H3A by 0.39 M KOH for the next three questions. The triprotic acid has Ka1= 1.0 x 10-3, Ka2 = 1.0 x 10-6, and an unknown value for Ka3. -Calculate the pH after 100.0 mL of KOH has been added. -Calculate the pH after 150.0 mL of KOH has been added. -The pH of the solution after 200.0 mL of KOH has been added is 8.00. Determine the value of Ka3 for this triprotic acid. Use scientific notation to enter this answer, e.g., 1.0 x 10-3 = 1.0E-3.
-4.50 -6 -1.0*10^-10
Fe2+ (aq) + 2e- → Fe (s) ξstandard =-0.44 Al3+ (aq) + 3e- → Al (s) ξstandard =-1.66 Calculate ∆Gstandard
-706.380kJ
consider 1.0 L of a solution which is 0.6M NH4Cl and 0.2M NH3 (Ka for NH4Cl = 5.6 x 10-10) -Calculate the pH of this solution. -Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change. -Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.
-8.77 -8.4 -9.25
For the reaction at 298 K, CH4 g + 2O2 g → CO2 g + 2H2O g the values of ΔH and ΔS are -803 kJ and -4.00 J/K, respectively. What is the value of ΔG?
-802 kJ
A first order reaction, where [A]initial = 1.00 M, is 69.5 % complete in 375 s. How long does it take for the same reaction to go from 1.00 M to 85.5 % completion?
610. s
Calculate the pH of a 0.79 M solution of BaBr2.
7.00
What mass of calcium metal is produced when molten CaF2 is electrolyzed by a current of 6.03 A for 17 h?
76.6 g
Calculate the pH of a 0.62 M solution of KNO2 (Ka for HNO2 = 4.0 x 10-4).
8.5952
For the reaction at 298 K, 2NO2 g → N2O4 g the values of ΔH and ΔS are -58.0 kJ and -177 J/K, respectively. What is the value of ΔG nonstandard at 298 K when the concentration of N2O4 is 1.71 M and the concentration of NO2 is 2.89 M?
9.18kJ
Consider the following reaction: A + B → C (slow) C → D D + E → F + B Label all reactants, products, intermediates, and catalysts in this reaction. What's the rate law?
A, E = reactants F = products B = catalyst C,D = intermediates rate=k[A][B]
Consider the following molecules: acetic acid (CH3COOH, Ka = 1.8 x 10-5), ammonia (NH3, Kb = 1.8 x 10-5), hypochlorous acid (HOCl, Ka = 2.9 x 10-8), and aniline (C6H5NH2, Kb = 3.8 x 10-10). Which of these molecules will exist in their ionic form at a pH of 3.00?
Acetic Acid - false Ammonia - true Hypochlorous acid - false Aniline - true
True or False: A secondary alkyl halide could react through either an SN1 or SN2 mechanism because backside attack is possible (albeit slow) and a secondary carbocation is relatively stable (which would give a similar rate of reaction as for SN2)
False
True or False: A successful collision (one that leads to the combustion of methane) will will not need to meet the activation energy due to the extreme exothermic nature of the reaction.
False
True or False: Anions flow towards the cathode
False
True or False: As a solution becomes more basic, the pOH of the solution increases
False
True or False: Copper metal is often used as an inert electrode
False
True or False: Electrons flow from the cathode to anode
False
True or False: Once the activation energy has been reached, increasing the temperature will have no effect on the rate of the reaction.
False
True or False: Reduction occurs at the anode
False
True or False: SN2 leads to a racemization of sterechemistry due to the planar carbocation intermediat
False
True or False: The conjugate base of a weak acid is a strong base.
False
True or False: for polyprotic acids Ka1 is typically much smaller than Ka2
False
True or False: ΔG is equal to the minimum non-expansion work that a system can perform
False
Go and do Orgo IV Problem 2
Go and do Orgo IV Problem 2
Go and do Orgo IV Problem 3
Go and do Orgo IV Problem 3
Go and do Orgo IV Problem 4
Go and do Orgo IV Problem 4
Go and do Toolbox 1 PL Question
Go and do Toolbox 1 PL Question
Go do GHW Acid base XII
Go do GHW Acid Base XII
Go do Kinetics II GHW problem 2
Go do Kinetics II GHW problem 2
Go do Kinetics II GHW problem 3
Go do Kinetics II GHW problem 3
Go do Orgo III Problem 1
Go do OrgoIII Problem 1
Go do SN1 SN2 Problem 1
Go do SN1 SN2 Problem 1
Go through Electrochem 0 GHW 1
Go through Electrochem 0 GHW 1
Go through Electrochem 0 GHW 2
Go through Electrochem 0 GHW 2
Go through Kinetics III Problem 2
Go through Kinetics III Problem 2
Go through Kinetics III Problem 3
Go through Kinetics III Problem 3
Go through Kinetics IV Problem 1
Go through Kinetics IV Problem 1
Go through Kinetics IV Problem 2
Go through Kinetics IV Problem 2
Go through Kinetics V Problem 1
Go through Kinetics V Problem 1
Go through Kinetics V Problem 2
Go through Kinetics V Problem 2
Go through Kinetics V Problem 3
Go through Kinetics V Problem 3
Go through Kinetics VI Problem 1
Go through Kinetics VI Problem 1
For 0.67 M HNO2 (Ka=4.0×10-4), mark the major species found in the solution.
H2O, HNO2
Given the following pair of half-reactions, fill in the line notation for a standard cell using these two half-reactions. Since it is a standard cell, all concentrations will be 1 M, so do not enter concentrations. You have solid platinum (Pt) electrodes to use, where necessary. F3- (aq) + 2e- → 3 F- (aq) ξo = 0.55 TF3+ (aq) + 2e- → TF+ (aq)ξo = 1.24
Pt | F3- F- || TF3+ TF+ | Pt
True or False: The Ka equilibrium constant always refers to the reaction of an acid with water to produce the conjugate base of the acid and the hydronium ion.
True
True or False: The cathode reagents are found to the right of the salt bridge
True
True or False: The line notation for a cell based on the balanced equation Cu2+ + Zn → Zn2+ + Cu would look like this: Zn| Zn2+ || Cu2| Cu
True
Based on the standard reduction potentials given below, which species is most likely to be oxidized? -Ag+ + e- → Ag, E= 0.80V -Cu2+ + 2e- → Cu, Eo=0.34V -Zn2+ + 2e- → Zn, Eo=-0.76V -Cd2+ + 2e- → Cd, Eo=-0.40V
Zn
For a 0.015 M solution of HNO3, calculate: [H+], pH, pOH, and [OH-]
[H+] = 0.015M pH = 1.82 pOH = 12.18 [OH-] = 6.7 * 10^-13
calculate: [H+], pH, pOH, and [OH-] for a 1.0×10−13 M solution of HI.
[H+] = 1.0*10^-7 pH = 7 pOH = 7 [OH] = 1.0*10^-7
For a 2.70 M solution of NaOH, calculate:[H+], pH, pOH, and [OH-]
[H+]= 3.70×10-15 pH= 14.43 pOH= -0.43 [OH-]= 2.70
Bronsted Lowry
acid-base reaction theory
What functional group is found in the structure for vitamin c?
ether
Does NO3- have a strong or weak conjugate acid?
strong conjugate acid
True or False: An inert electrode can be used in the anode or cathode (if needed)
True
True or False: An inert electrode is needed when there is no conducting solid to attach a wire to
True
True or False: As the Kb value for a base increases, base strength increases.
True
True or False: For most polyprotic acids Ka1 largely determines the pH of the solution
True
True or False: For most polyprotic acids, each proton dissociation can be looked at separately
True
True or False: Having a greater number of electron withdrawing groups is typically the best way to stabilize a conjugate base
True
True or False: If R-3-bromo-3-methylhexane is allowed to react with OH- the product will be a 50%/50% mixture of R-3-methyl-3-hexanol and S-3-methyl-3-hexanol
True
True or False: In a galvanic cell, electrons are spontaneously produced in the lead half-cell.
True
True or False: Once the activation energy has been reached increasing the concentration of methane and oxygen will increase the rate of the reaction.
True
True or False: Reduction occurs at the cathode
True
True or False: SN1 leads to a racemization of sterechemistry due to the planar carbocation intermediate
True
True or False: Standard reduction potential is an intensive property
True
Does C3H5O2- have a strong or weak conjugate acid?
weak conjugate acid
Does CN- have a strong or weak conjugate acid?
weak conjugate acid
Does NH3 have a strong or weak conjugate acid?
weak conjugate acid
True or False :A spontaneous electrochemical reaction will always have a negative voltage
False
True or False: A positive value for ΔG means equilibrium will lie towards the products
False
Consider the generic reaction below: A (aq) + 2 B (aq) ⇌ C (aq) + D (aq) Where ΔG standard is -10.2 kJ for the reaction -The value of ΔG standard is the amount of energy free to do work under any conditions -ΔG nonstandard allows us to determine the equilibrium constant, K, for the reaction -If the reaction shown is at equilibrium, ΔG nonstandard is equal to zero -This reaction will always be spontaneous because ΔG standard is negative
-False -False -True -False
Cu2+(aq) + 2 e- → Cu (s)+ 0.34 Zn2+(aq) + 2 e-→ Zn (s)- 0.76 -the solid metal cathode decreases by mass -Positively charged ions flow from the salt bridge to the anode. -The concentration of Cu2+ decreases as the reaction proceeds. -Cu2+ is a reactant of this overall reaction. -Adding more Zn2+ will favor the reverse reaction.
-False -False -True -True -True
Consider a buffer solution consisting of CH3NH3Cl and CH3NH2. Which of the following statements are true concerning this solution?(Ka for CH3NH3+ = 2.3 x 10 -11). - If HCl were added to the initial buffer solution, then the [CH3NH3+] would decrease. -If [CH3NH3+] = [CH3NH2], then pH = 10.64. - A solution consisting of 0.1 M CH3NH3Cl and 0.1 M CH3NH2 would be a more effective buffer than one containing 1.5 M CH3NH3Cl and 1.5 M CH3NH2 -Adding more [CH3NH3+] to the initial buffer solution will decrease the pH. -If [CH3NH3+] > [CH3NH2], then the [H+] is smaller than the Ka value. -If [CH3NH3+] >[CH3NH2], then pH is larger than the pKa
-False -True -False -True -False -False
Which of the following compounds contain at least one stereogenic center? -methylcyclopentane -2,3-dimethylhexane -1,2-dimethylcyclopentane -2-methylhexane
-False -True -True -False
R-X + OH- → R-OH + X- -1-chloro-3-methylbutane -3-chloro-2,2-dimethylbutane -2-chloro-2-methylpropane -3-chloro-3-ethylpentane
-SN2 -more info needed -SN1 -SN1
Calculate the pH of a 0.15 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x 10-9).
3.027
The rate law for the reaction O2 (g) + 2 NO (g) → 2 NO2 (g) is rate = k[NO]2[O2]. Which of the following will lead to a change in the rate constant, k? -The catalyst is removed from the reaction -The volume of the container is cut by 1/4 -The temperature of the reaction is increased -The pressure of NO is doubled
-The catalyst is removed from the reaction -The temperature of the reaction is increased
The spontaneity of a standard reaction, ΔG standard, depends on both ΔH and ΔS. Given the following reaction and data table, decide if each of the statements shown below are True or False. Assume that ΔH and ΔS are independent of Temperature. -CCl4 (l) → C (gr) + 2 Cl2 (g) -ΔHrxn = 136 kJ -ΔSrxn = 235 J/K -This reaction is endothermic -This reaction is exothermic -This reaction is endergonic (ΔG > 0) at 298K -This reaction is exergonic (ΔG < 0) at 298K -This standard reaction will only be spontaneous at high temperatures (T >579K) -This standard reaction will only be spontaneous at low temperatures (T < 579 K) -This standard reaction will be spontaneous at all temperatures -This standard reaction will not be spontaneous at any temperature
-True -False -True -False -True -False -False -False
Will the following reactions show an increase or decrease for the value of ΔSrxn? -CO2 g → CO2 s -2CH3OH g + 3O2 g → 2CO2 g + 4H2O g -Ag+ aq + Cl- aq → AgCl s -2H2 g + C s → CH4 g
-decrease -increase -decrease -decrease
Consider a solution of 0.60 M C5H5N (Kb = 1.7×10-9). Decide if each of the following is a major or minor species in the solution. -H2O -C5H5NH+ -OH- -C5H5N -H+ -Calculate the pH of this solution.
-major -minor -minor -major -minor -9.50
For each salt, indicate whether the solution is acidic, basic, or neutral. -NaCl -RbOCl -CsF -Ca(NO3)2 -H2NNH3Cl -C2H5NH3NO3
-neutral -basic -basic -neutral -acidic -acidic
Given the following values of ΔS universe predict if a reaction will be spontaneous, non-spontaneous, or at equilibrium. -Delta S Universe is positive -Delta S Universe is 0 -Delta S Universe is Negative
-spontaneous -equilibrium -not spontaneous
Consider the titration of 0.100 L of 0.300 M acetic acid with 2.50 M NaOH. What type of calculation will we be performing at the following points of the titration curve? -1.4 equivalents of base added -Zero equivalents of base added -One equivalent of base added -0.6 equivalents of base added
-strong base calculation -weak acid calculation -conjugate base calculation -buffer calculation
Determine the pH of a buffer solution comprised of a 1.19 M HF and 0.929 M NaF. The Ka of HF = 7.20 x 10-4.
3.03
Consider a buffer made from a solution of HF to which has been added NaF. The Ka of HF is 7.20 x 10-4. Given what you know about the Henderson-Hasselbalch equation determine if each of the following statements is true or false. -When [HF] = [F-] = 1.0 M, the buffer will resist pH change better than if [HF] = [F-] = 0.10 M -This specific system could be used to buffer a solution at a pH of 2.0 -F- is the "HA" species in the Henderson-Hasselbalch equation -When [HF] = [F-], the pH of the buffer will always be 3.14
-true -false -false -true
What is the entropy (S) of a perfect crystal at 0K
0
Theophylline is a pharmaceutical drug that is sometimes used to help with lung function. You observe a case where the lab results indicate that a sample of theophylline (initial concentration of 2.0 x 10-3 M) has been metabolized to a concentration of 1.0 x 10-3 M in 24 hours. In another 24 hours the drug concentration was 5.0 x 10-4 M. What is the rate of decomposition four (4) hours after the initial sample was taken?
0.00005146
Consider the cell described below at 255 K: Sn | Sn2+ (0.945 M) || Pb2+ (0.967 M) | Pb Given Estandard of Pb2+→Pb = -0.131 V, Estandard of Sn2+→Sn = -0.143 V. Calculate the cell potential after the reaction has operated long enough for the Sn2+ to have changed by 0.333 mol/L.
0.0043V
ClO3-(aq) + 9I- (aq)+ 6 H+ (aq) → 3I-3 (aq) + Cl-(aq) + 3H2O If the initial rate of disappearance of I- under a given set of experimental conditions is 32.8 x 10-3 M/s then what is the rate of disappearance of H+ under those same experimental conditions?
0.0219 M/s
Calculate the pH of a 0.717 M solution of HNO3
0.144
Consider the cell described below at 298K: Fe | Fe3+ (2.00 M) || Cu2+ (1.00 M), Cu+ (0.600 M) | Pt Calculate the cell potential after the reaction has operated long enough for the [Fe3+] to have changed by 0.200 M.
0.161
Consider the following reaction at 289 K: 2A + B → C + D Where rate = k[A][B]2. An experiment was performed where [A]initial = 2.99 M and [B]initial = 0.00235 M. A plot of 1/[B] vs. time has a slope of 10.01 s-1. What will the rate of this reaction be when [A] = [B] = 0.397 M?
0.209 M/s
If an aqueous solution of HNO3 is electrolyzed for 29.00 min at a steady current of 1.63 A, what volume of H2 (g) at 25.0oC and 1.01 atm will be collected at the cathode?
0.356L
Consider the Molecular Orbital diagram for the ion H2- (An H2 ion with 3 e-). Predict the bond order. Will the ion be paramagnetic or diamagnetic?
0.5 paramagnetic
Use the following pair of reduction half-reactions to design a galvanic cell. Then write in the proper coefficient for each of the species involved in the overall reaction. Water molecules and protons are not shown in the half-reactions, but may be needed in the overall reaction. MnO4- (aq)→MnO2 (s)ξo = 0.59 V NO3- (aq)→NO (g)ξo = 0.96 V -NO3- (aq) -MnO4- (aq) -NO (g) -MnO2 (s) -H+ (aq) -H2O (l)
1,1,1,1,0,0
Rank the following chemical species from lowest absolute entropy (So) (1) to highest absolute entropy (5) at 298 K? -H2O (l) -Ca (s) -C2H6 (g) -Al (s) -HF (g)
3,2,5,1,4
Rank the following chemical species from lowest absolute entropy (So) (1) to highest absolute entropy (5) at 298 K? -CH3COOH (l) -HCN (g) -Al (s) -Ca (s) -C2H6 (g)
3,4,1,2,5
Rank the following titrations in order of increasing pH at the equivalence point of the titration (1 = lowest pH and 5 = highest pH). -100.0 mL of 0.100 M KOH by 0.100 M HCl -200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH -100.0 mL of 0.100 M NH3 (Kb = 1.8 x1 0-5) by 0.100 M HCl -100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl -100.0 mL of 0.100 M HNO2 (Ka = 4.0 x 10-4) by 0.100 M NaOH
3,5,1,2,4
Consider the Molecular Orbital diagram for the ion O22-. Predict the bond order. Which type of orbital will be the lowest unoccupied molecular orbital (LUMO)? Which type of orbital will be the highest occupied molecular orbital (HOMO)? Will the ion be paramagnetic or diamagnetic?
1.0 Pσ* (P sigma star) Pπ* (P pi star) diamagnetic
Given the two following half reactions: Cu2+ + 2 e- → Cu SRPo = 0.34 V Zn2+ + 2 e- → Zn SRPo = -0.76 V Determine the potential of the cell when Zn2+ has changed by 0.3 M.
1.1079
2NO2 → 2NO + O2. obeys the rate law: rate = 1.4 x 10-2[NO2]2 at 500 K. What would be the rate constant at 227 K if the activation energy is 80. kJ/mol?
1.24e-12
Calculate how many grams of gold would be plated out on a coin, if a current of 1.7 (Amp) is applied for 18 min to an electrolytic cell shown above.The following reaction is occurring: Au3+ + 3 e- → Au
1.25 g
Calculate the pH of the 0.67 M HNO2 solution (Ka= 4.0×10-4).
1.79
What is the pH of a 227 mL sample of 2.427 M benzoic acid (C6H5COOH) (Ka = 6.4 x 10-5)?
1.90
Consider the reaction: 3A + B + 2 C → D + E where rate = k[A]2[C]2. A reaction was performed where [B]initial = [C]initial = 0.700 M and [A]initial = 3.20 x 10-5 M. A plot of 1/[A] vs time (min) gave a plot with a straight line relationship and after 7.00 min, [A] = 1.70 x 10-6 M. What will the rate of reaction be when [A] = [B] = [C] = 0.170 M?
135.63
Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). -200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH -100.0 mL of 0.100 M HI by 0.100 M NaOH -100.0 mL of 0.100 M NH3 (Kb = 1.8 x1 0-5) by 0.100 M HCl -100.0 mL of 0.100 M KOH by 0.100 M HCl -100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl
2,1,3,5,4
N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation (∆Gf) of NH3 (g) is -111 kJ/mol at 338 K, calculate the equilibrium constant, K, at this temperature
2.04e34
You have a 4.14E-3 M solution of [H+], what is the concentration of [OH-] in the sample?
2.42×10-12
The rate constant for a first order reaction is 0.060. when the temperature is increased from 298K to 302 K , the rate constant increases to 0.18. Calculate the activation energy for this reaction.
205.5 kJ
Use the values of S (J) given below to calculate ∆So for the following reaction: C2H5OH(l) + 3O2(g) → 2CO2(g)+ 3H2O(g) -C2H5OH (l) = 161 -O2 (g) = 205 -CO2 (g) = 213.6 -H2O (g) = 188.7
217.3 J
Use the values of ∆Gf (kJ) given below to calculate ∆Grxn for the following reaction2 Na (s) + 2 H2O (l) → 2 NaOH (aq)+ H2 (g) -Na (s) = 0 -H2O (l) = -237.2 -NaOH (aq) = -419.2 -H2 (g) = 0.0
364 kJ
Calculate the boiling point of formic acid, CHOOH from the data given below:-CHOOH (l) → CHOOH (g) -CHOOH (l) = Delta S 129 J, Delta H -409.8(kJ) -CHOOH (g) = Delta S 251 J, Delta H -362.6kJ
386.9K
Balance the following redox reaction and enter the correct coefficients for all of the species in the balanced reaction. SO2 (aq) + MnO4- (aq) → SO42- (aq) + Mn2+ (aq) This reaction takes place in an acidic solution -SO2 (aq) -H2O -Mn2+ -MnO4- - SO42- - H+
5,2,2,2,5,4
Which of the following definition of a Bronsted-Lowry Acid is most accurate -A Bronsted-Lowry acid is an electron pair donor -A Bronsted-Lowry acid always dissociates completely in water -A Bronsted-Lowry acid is an electron pair acceptor -A Bronsted-Lowry acid is a proton acceptor -A Bronsted-Lowry acid is a proton donor
A Bronsted-Lowry acid is a proton donor
What is the conjugate base of HBr?
Br-
Pb2+ + 2 e- → Pb (s) ξo = -0.13 V Ag+ + 1 e- → Ag (s) ξo = 0.80 V What is the voltage, at 298 K, of this voltaic cell starting with the following non-standard concentrations:[Pb2+] (aq) = 0.099 M[Ag+] (aq) = 0.61 M
E = 0.95V
Arrange KClO4, HCl, RbOCl, C6H5NH3Cl, and Ba(OH)2 from lowest to highest pH
HCl < C6H5NH3Cl < KClO4 < RbOCl < Ba(OH)2
Rank the solutions in order of increasing pH where 1 is the solution with the lowest pH and 7 is the solution with the highest pH. KNO3, C6H5NH2, H3BO3, Ca(OBr)2, NaOH, HCl, H2NNH3Cl
HCl< H2NNH3Cl < H3BO3 < KNO3 < C6H5NH2 < Ca(OBr)2 < NaOH
Rank the following 0.10 M solutions in order of increasing pH: C5H5N, NaCl, NaOH, HNO3, HCN
HNO3 < HCN < NaCl < C5H5N < NaOH
Rank the following 0.10 M solutions in order of increasing pH HNO2, HNO3, NaCl, HC2H3O2
HNO3 < HNO2 < HC2H3O2 < NaCl
What is the conjugate base of HPO4 2-?
HPO4 3-
What is the conjugate base of HSO4-?
HSO4 2-
Calculate the equilibrium constant, Ka for the acid, HA if, at equilibrium, the pH of a 2.00 M solution of HA is 2.77?
Ka = 1.44×10-6
A 0.100 M solution of an unknown acid, HA, is 1.96% ionized. What is the Ka of HA? Now calculate the pH of the solution of HA.
Ka = 3.92×10-5 pH = pH= 2.71
What is the conjugate base of HNO3?
NO3-
Consider the following acids and bases: HCO2H: Ka=1.8x10-4 HOBr: Ka=2.0x10-9 HONH2: Kb=1.1x10-8 (C2H5)2NH: Kb=1.3x10-3 Which one combined with its conjugate would give the best buffer solution with a pH of 9?
NaOBr HOBr
True or False: 1-bromopentane will undergo substitution through an SN1 mechanism
True
True or False: A mixture of methane and oxygen can be kept in the same container indefinitely at room temperature with no change because the collisions taking place between the molecules do not have enough energy to reach overcome the reaction barrier.
True
Toolbox 1 GHW problem 1
Toolbox 1 GHW problem 1
Toolbox 1 GHW problem 2
Toolbox 1 GHW problem 2
Toolbox 1 GHW problem 3
Toolbox 1 GHW problem 3
Toolbox 2 GHW problem 1
Toolbox 2 GHW problem 1
Toolbox 2 GHW problem 2
Toolbox 2 GHW problem 2
Toolbox 2 GHW problem 3
Toolbox 2 GHW problem 3
Toolbox 2 GHW problem 4
Toolbox 2 GHW problem 4
Draw out 4-ethyl-3-isopropyl-2,5-dimethylheptane
Toolbox 2 GHW problem 5
Draw out 5-tert-butyl-6-isopropyl-3-methylnonane
Toolbox 2 GHW problem 5
Toolbox 2 GHW problem 5
Toolbox 2 GHW problem 5
Toolbox 2 GHW problem 6
Toolbox 2 GHW problem 6
True or False: A negative value for ΔG standard means a reaction is spontaneous under standard conditions
True