chem final
which of the following liquids would you expect to have the lowest vapor pressure at room temperature? Ethylene glycol (198 degrees celcius bp) Ethanol (78.3 degrees celcius bp) Benzene (80 degrees celcius bp) n-pentane (36.1 degrees celcius bp) Chloroform (62 degrees celcius bp)
Ethylene glycol (198 degrees celcius bp)
As pure molecular solids, which of the following exhibits dipole-dipole intermolecular forces: HBr, NBr3, SBr2, and CBr4
HBr, NBr3, and SBr2
calculate delta G for the reaction at 425 degrees celcius: 2 HI(g)=H2(g)+I2(g); K=0.018. (R=8.314 J/K*mol)
23.3 kj/mol-rxn
at a given temperature, K=0.034 for the equilibrium PCl5(g)=PCl3(g)+Cl2(g) what is K for: Cl2(g)+PCl3(g)=PCl5(g)?
29
what is the mole fraction of urea, CO(NH2)2 (MW=60.6 g/mol), in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol, CH3OH (MW=32.04 g/mol)?
0.078
for the second-order reaction below, the initial concentration of reactant A is 0.24 M. if the rate constant for the reaction is 1.5x10^-2 M^-1s^-1, what is the concentration of A after 265 seconds? 2A=B+C. rate=k[A]^2
0.12 M
calculate the standard cell potential, Ecell, for the reaction 2Li(s)+Ba^2+(aq)=2Li^+(aq)+Ba(s) the standard reduction potentials are as follows: Li^+(aq)+e^-=Li(s). Ecell=-3.040 V Ba^2+(aq)+2E^-=Ba(s). Ecell=-2.912 V
0.128V
assuming ideal behavior, which of the following solutions would have the highest osmotic pressure? 0.2 M KBr 0.3 M CH3COOH 0.3 M C12H22O11 0.2 M CaCl2 0.3 M C6H12O6
0.2 M CaCl2
what is the mole fraction of urea, CH4N2O (MW=60.06 g/mol), in an aqueous solution that is 46% urea by mass?
0.20
if 0.357 g of CH4 gas is introduced into an empty 1.75 L flask at 25 degrees celcius, what will be the pressure inside the flask?
0.311 atm
the partial pressures of CH4, N2, and O2 in a sample of gas mixture were found to be 143 mm Hg, 466 mm Hg, and 591 mm Hg, respectively. calculate the mole fraction of nitrogen.
0.388
for the equilibrium PCl5(g)=PCl3(g)+Cl2(g), Kc=4.0 at 228 degrees celcius. if pure PCl5 is placed in a 1.00L container and allowed to come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.11 M, what is the equilibrium concentration of PCl3?
0.66 M
at 25 degrees celcius, all of the following ions produce an acidic solution, except: 1. HPO4^2- 2. [Al(H2O)6]^3+ 3. NH4^+ 4. HSO^3- 5. [Fe(H2O)6]^3+
1
calculate the Ka values for the following acids: 1. cyanic acid, HOCN, 3.5x10^-4 2. formic acid, HCHO2, 1.7x10^-4 3. lactic acid, HC3H5O3, 1.3x10^-4 4. propionic acid, HC3H5O2, 1.3x10^-5 which is the strongest acid?
1
for which of the following reactions will entropy of a system decrease? 1. 2 NO2(g)=N2O4(g) 2. 2 NH3(g)=N2(g)+3 H2(g) 3. CaCO3(s)=CaO(s)+CO2(g) 4. NaOH(s)=Na^+(aq)+OH^-(aq)
1
all of the following compounds are acids containing chlorine. Which is the weakest acid? 1. HCl 2. HClO4 3. HClO
3
an acid base system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. what is the effect of adding 0.50 mol CH3CO2^2-(aq) to this solution? 1. the pH of the solution will equal 7.00 because the equal concentrations of a weak acid and its conjugate base are present. 2. some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2^-(aq) and increasing the pH. 3. Some CH3CO2^-(aq) will react with H3O^+, increasing the concentration of CH3CO2H(aq) and reestablishing the solution equilibrium.
3
calculate the Ka values for the following acids: 1. cyanic acid, HOCN, 3.5x10^-4 2. formic acid, HCHO2, 1.7x10^-4 3. lactic acid, HC3H5O3, 1.3x10^-4 4. propionic acid, HC3H5O2, 1.3x10^-5 initially equimolar solutions of each weak acid, which solution will have the lowest hydronium ion concentration once equilibrium is established?
3
in which of the following solutions silver (I) phosphate, Ag3PO4, be least soluble 1. 0.10 M Na2HPO4 2. 0.10 M NaH2PO4 3. 0.10 M AgNO3 4. 0.10 M HNO3 5. 0.10 M Na3PO4
3
use the following standard reduction potentials to determine which species is the strongest oxidizing agent. 1. Fe^2+(aq)+2E^-=Fe(s). E=-0.41 V 2. Cu^2+(aq)+2E^-=Cu(s). E=0.34 V 3. Cr2O7^2-(aq)+14H^+(aq)+6^E^-=2Cr^3+(aq)+7H2O(l). E=1.33 V
3
which of the following is true concerning a reaction that is product favored? 1. Q=K AND DELTAG=0 2. Q<K AND DELTA G>0 3. Q<K AND DELTA G<0 4. Q>K AND DELTA G>0
3
which of the following statements regarding entropy is/are true? 1. the entropy os a substance increases when converted from a liquid to a solid 2. the entropy of a substance decreases as its temperature increases 3. all substances have positive entropy values at temperatures above 0 K.
3
which of the following statements concerning real gases is/are correct? 1. real gases are always liquids or solids at temperatures below 273.15 K. 2. the pressure of a real gas is higher than predicted by the ideal gas law. 3. the molecules in a real gas are attracted to each other.
3 only
a 50.00mL solution of 0.0350 M aniline (Kb=3.8x10^-10) is titrated with a 0.0113 M solution of hydrochloric acid as the titrant. what is the pH at the equivalence point? (Kw=1.0x10^-14)
3.32
the mechanism of a chemical reaction is given below. (CH3)3CCl=(CH3)3^++Cl^- (slow) (CH3)3C^++OH^-=(CH3)3COH (fast) which of the following statements concerning the reaction is/are correct? 1. the overall balanced reaction is: (CH3)3CCl+OH^-=(CH3)3COH+Cl^- 2. hydroxide ion is a reaction intermediate 3. the following rate law is consistent with the mechanism: rate=k[(CH3)3CCl][OH^-]
1
which equation depicts the hydrogen phosphate ion behaving as a bronsted lowry base in water 1. HPO4^2-(aq)+H2O(l)=H2PO4^-(aq)+OH^-(aq) 2. HPO4^2-(aq)+OH^-(aq)=PO4^-(aq)+H2O(l) 3. 2 HPO4^2-(aq)+H2O(l)=2 H2O(l)+P2O7(s) 4. 2 HPO4^2-(aq)+O^2-(aq)=PO4^3-(aq)+H2O(l)
1
which of the following statements is/are correct? 1. a unit cell is the smallest repeating unit that has all of the symmetry characteristics of the arrangement of atoms, ions, or molecules in a solid. 2. transition metals with high densities, especially those in period 6, preferentially crystallize with a primitive cubic cell structure. 3. the preferred crystal structure of the group 1a metals is face centered cubic.
1
the concentration of magnesium carbonate is a saturated aqueous solution at 25 degrees celcius is 1.9x10^-4 M. what is the Ksp of this sparingly soluble salt?
3.5x10^-8
which of the following statements is/are true with the Bronsted-Lowry concept of acids and bases? 1. a conjugate acid-base pair consists of two species that may differ by one proton. 2. a bronsted lowery base is defined as a hydroxide ion donor. 3. bronsted lowry acid-base reactions are restricted only to aqueous solutions.
1
a solution is prepared by dissolving 5.88 g of an unknown non-electrolyte in enough water to make 0.355 L of solution. the osmotic pressure of the solution is 1.21 atm at 27 degrees celcius. what is the molar mass of the solute? (R=0.08206 Latm/molK)
337 g/mol
calculate the value deltaG for the following redox reaction: Fe^3+(aq)+2Cl^-(aq)=Fe(s)+Cl2(g). Ecell=-1.80V
347 kJ/mol-rxn
write a balanced chemical equation for the redox reaction in basic solution. ClO^-(aq)+Cr(OH)3(s)=Cl^-(aq)+CrO4^2-(aq)
3ClO^-(aq)+2Cr(OH)3(s)+4OH^-(aq)=3Cl^-(aq)+2CrO4^2-(aq)+5H2O(l)
for which of the following reactions is Kc=Kp? 1. CaO(s)+CO2(g)=CaCO3(s) 2. CO(g)+H2(g)=CH4(g)+H2O(g) 3. HBr(g)=1/2H2(g)+1/2Br2(l) 4. CO(g)+H2O(g)=CO3(g)+H2(g)
4
a gaseous mixture containing 1.5 mol Ar and 3.5 mol CO2 has a total pressure of 6.1 atm. what is the partial pressure of CO2?
4.3 atm
what is the molar solubility of silver(I) acetate at 25 degrees celcius? the solubility product constant for silver (I) acetate is 2.0x10^-1 at 25 degrees celcius.
4.5x10^-2 M
the concentration of calcium carbonate in a saturated aqueous solution at 25 degrees celcius is 6.7x10^-4 M. what is the Ksp of this sparingly soluble salt?
4.5x10^-9 M
the henry's law constant for N2 in water at 25 degrees celcius is 6.0x10^-4 mol/kgbar. what is the equilibrium concentration of N2 in water when the partial pressure of N2 is 586 mm Hg (760 mm Hg=1 atm=0.9869 bar; assume the density of the solution is 1.00 g/mL)
4.6x10^-4 M
the molar mass of an unknown gas was measured by an effusion experiment. it was found that the unknown gas effused at a rate of 2.7x10^-6 mol/hr, whereas the nitrogen gas effused at a rate of 3.3x10^-6 mol/hr. the molar mass of the gas is?
42 g/mol
the heat of vaporization of benzene (C6H6) is 30.7 kJ/mol at its boiling point of 80.1 degrees celcius. how much energy in the form of heat is required to vaporize 112 g benzene at its boiling point?
44.0 kJ
calculate the root mean square velocity for the O2 molecules in a sample of O2 gas at 16.3 degrees celcius.
474.9 m/s
all of the following statements concerning acid-base buffers are true EXCEPT: 1. the pH of a buffer is close to the pKa of the weak acid from which it was made 2. buffers are resistant to pH changes upon addition of small quantities of strong acids or bases 3. buffers are resistant to changes in pH when diluted with water 4. buffers contain appreciable quantities of a weak acid and its conjugate base 5. buffers are used as colored indicators in acid base titrations
5
which of the following changes leads to a decrease in entropy? 1. mixing of pure gases 2. decomposition of fallen leaves 3. melting snow 4. boiling water 5. rain drops forming in a cloud
5
which of the following ionic compounds forms a neutral aqueous solution at 25 degrees celcius? 1. NH4F 2. NaHCO3 3. K2S 4. KCN 5. LiI
5
the vapor pressure of pure water at 15 degrees celcius is 12.8 mm Hg. what is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol, CH3CH2OH (MW=46.07 g/mol) and 22.0 g water?
5.61 mm Hg
consider the reaction NH3(aq)+H2O(l)=NH4^+(aq)+OH^-(aq). Kb for NH3 is 1.8x10^-5 at 25 degrees celcius. what is the Ka for the NH4^+ ion at the same temperature?
5.6x10^-10
at a given temperature, 0.0664 mol N2O4(g) is placed in a 1.00 L flask. After reaching equilibrium, the concentration of NO2(g) is 6.1x10^-3 M. What is Kc for the reaction below? N2O4(g)=2NO2(g)
5.9x10^-4
for the reaction N2O4(g)=2NO2(g), Kp=0.148 at a temperature of 298 K. what is Kp for the following reaction? 14NO2(g)7N2O4(g)
6.43x10^5
the Ksp of silver bromide is 5.4x10^-13 at 298 K. AgBr(s)=Ag^+(aq)+Br^-(aq) what is delta G for reaction? (R=8.314 J/K*mol)
7.0x10^1 kJ/mol
what is the pH of a buffer composed of 0.35 M H2PO4^-(aq) and 0.65 M HPO4^2-(aq)? (Ka of H2PO4^- is 6.2x10^-8)
7.48
a 50.00mL solution of 0.0610 M hydrofluoric acid (Ka=7.2x10^-4) is titrated with 0.0209 M solution of NaOH as the titrant. what is the pH of at the equivalence point? (Kw=1.00x10^-14)
7.67
the equilibrium constant Ka for the monoprotic acid, proprionic acid is 1.3x10^-5. which of the following is the correct value of Kb for the propionate ion, the conjugate base of propionic acid?
7.7x10^-10
the pressure of O2 in a 15.0 L flask is 322 mm Hg at 44 degrees celcius. what mass of O2 is in the flask? (R=0.08206 L*atm/mol*K)
7.82 g
cesium bromide crystallizes in a primitive cubic unit cell with bromide ions at each corner and a cesium ion occupying the cubic hole. what is the coordination number of the cesium in this structure?
8
in a first-order reaction, the half life is 134 minutes. what is the rate constant?
8.62E-5s^-1
the H3O^+ concentration of a solution is 5.6x10^-6 M. what is the pOH of the solution?
8.75
what is the pH of an aqueous solution composed of 0.64 M NH4^+ and 0.20 M NH3? (Ka of NH4+=5.6x10^-10)
8.75
what is the molar solubility of silver(I) iodide at 25 degrees celcius? the solubility product constant for silver(I) iodide is 8.3x10^-17 at 25 degrees celcius.
9.1x10^-9 M
nitrogen and oxygen gases may react to form nitrogen monoxide. at 1500 degrees celcius, Kc equals 1.0x10^-5 N2(g)+O2(g)=2NO(g) if 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L at 1500 degrees celcius, what is the concentration of NO(g) when equilibrium is established?
9.5x10^-5 M
which of the following correctly describes the influence of intermolecular forces on the properties of matter? 1. intermolecular forces determine the solubility of gases, liquids, and solids in various solvents. 2. intermolecular forces are directly related to the energy required to accomplish phase changes. 3. intermolecular forces do not influence the structure of molecules like DNA and proteins.
1 and 2
which of the following is/are expected to increase the rate of the exothermic combustion of coal? 1. using smaller pieces of coal. 2. increasing the concentration of oxygen. 3. lowering the temperature.
1 and 2
which of the following are valid reasons why vegetable oil has a greater viscosity than diethyl ether, CH3OCH3? 1. oil molecules have long chains that become entangled. 2. unlike diethyl ether, oil molecules are not held together by hydrogen bonds. 3. intermolecular forces are greater for the larger oil molecules.
1 and 3
which of the following statements concerning solubility is/are correct? 1. ionic compounds composed of group 1a metal ions and halide ions, such as NaCl, are insoluble in nonpolar solvents. 2. the solubility of halogens (Cl2, Br2, and I2) in polar solvents is greater than their solubility in nonpolar solvents. 3. the solubility of polar molecules, such as sugar, in polar solvents is generally greater than their solubility in nonpolar solvents.
1 and 3
which of the following statements is/are correct? 1. spontaneous changes only occur in the direction towards equilibrium 2. exothermic reactions are always spontaneous 3. in any chemical reaction, energy must be conserved
1 and 3
which of the statements concerning the phase diagram is/are correct? (basic unlabeled phase diagram) 1. only the solid phase exists at point a. 2. at point c, the solid and liquid phases are in equilibrium. 3. at point d, the critical point, the substance exists as a supercritical fluid.
1 only
which of the following statements are/is true? 1. oxidation occurs at an anode. 2. a spontaneous reaction generates an electric current in a voltaic cell 3. without a salt bridge, charge buildup will cause the cell reaction to stop
1, 2, 3
which of the following correctly describes the states of matter and intermolecular forces? 1. the change in volume that accompanies the conversion of a liquid to a gas can be very large. 2. the change in volume that accompanies the conversion of a liquid to a solid is small. 3. the forces of attraction between molecules in the liquid and solid state correlate with melting point, boiling point, and the energy of phase changes.
1, 2, and 3
what is the effect of adding an aqueous sodium hydroxide solution to an aqueous solution of ammonia? 1. the pH of the solution will increase 2. the concentration of NH4+(aq) will decrease 3. the concentration of NH3(aq) will increase
1,2, 3
a first-order chemical reaction is observed to have a rate constant of 32 min^-1. what is the corresponding half-life for the reaction?
1.3 s
for the first-rate decomposition of N2O5 at a high temperature, determine the rate constant if the N2O5 concentration decreases from 1.04M to 0.62M in 375 seconds.
1.38x10^-3 s^-1
at 80.0 degrees celcius water has an equilibrium vapor pressure of 355.1 mm Hg. if 4.22 g of H2O is sealed in an evacuated 5.00 L flask and heated to 80.0 degrees celcius, what mass of H2O will be found in the gas phase when liquid-vapor equilibrium is established? assume any liquid remaining in the flask has a negligible volume.
1.45 g
calculate standard reduction potential, Ecell, for the cell for the reaction 2Al(s)+3Sn^4+(aq)=3Sn^2+(aq)+2Al^3+(aq) standard reduction potentials are as follows: Al^3+(aq)+3E^-=Al(s). E=-1.66 V Sn^4+(aq)+2E^-=Sn^2+(aq). E=0.15 V
1.81 V
what is the equilibrium pOH of an initially 5.2 M solution of hypochlorous acid, HOCl, at 25 degrees celcius (Ka=3x10^-8)?
10.60
the average rate of disappearance of ozone in the following reaction is found to be 8.93x10^-3 atm/s. 2O3(g)=3O2(g) what is the rate of appearance of O2 during this interval?
13.4x10^-3 atm/s
if 27.9 g LiCl is dissolved in 175 g H2O, what is the weight percent of LiCl in the solution?
13.8%
sodium azide (FW=65.01 g/mol) decomposes rapidly to produce nitrogen gas by the following balanced equation: 2 NaN3 (s) = 2 Na (s) + 3 N2 (g) what mass of sodium azide totally decomposing will produce enough nitrogen to inflate a 60.0 L airbag for a car to a pressure of 1.50 atm at 305 K?
156 g
Gold crystallizes in a face-centered cubic lattice with an edge length of 407.8 pm. What is the density of gold?
19.3 g/cm^3
a catalyst [ ]. 1 is always a solid 2 changes the activation energy of the reaction 3 changes the potential energy of the reaction 4 does not influence the reaction in any way 5 is used up in a chemical reaction
2
determine which species is the strongest reducing agent: 1. 2 H^+(aq)+2 e^-=H2(g). E=0.00 V 2. K^+(aq)+e^-=K(s). E=-2.93 V 3. Al^3+(aq)+3e^-=Al(s). E=-1.66 V
2
for which of the following reactions is Kp=Kc? 1. NH3(g)=3/2H2(g)+1/2N2(g) 2. CH4(g)+2O2(g)=CO2(g)+2H2O(g) 3. C(s)+H2O(g)=H2(g)+CO(g)
2
in which of the following reactions does a decrease in the volume of the reaction vessel at a constant temperature favor the formation of the products? 1. H2(g)+I2(g)=2HI(g) 2. 2H2(g)+O2(g)=2H2O(g) 3. MgCO3(s)=MgO(s)+CO2(g)
2
when mixed in appropriate amounts, each of the following mixtures can produce an effective buffer solution except [ ]. 1. NaH2PO4 and Na2HPO4 2. NaOH and NaF 3. HCl and NaH2PO4
2
which of the following is/are expected to increase the rate of a chemical reaction? 1. decreasing the reactant concentrations 2. increasing the available surface area of a reactant 3. shaking a well mixed reaction solution
2
which of the following is/are physical properties of amorphous solids? 1. amorphous solids have well-defined melting points 2. at the particulate level, amorphous solids do not have long range order. 3. polymeric materials never form amorphous solids.
2
which of the following statements concerning the spontaneity of chemical and physical changes is correct? 1. a process can sometimes be spontaneous in the direction away from equilibrium 2. spontaneous changes occur only towards equilibrium 3. endothermic processes are never spontaneous 4. a reaction can't be spontaneous in more than one direction 5. a reactant favored process can not be spontaneous
2
what is the pH of a 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25 degrees celcius (Ka=7.8x10^-8)
2.10
a certain person has a body temperature of 309 K. on a cold day, what volume of air at 263 K must this person with a lung capacity of 2.5 L breathe in to fill his lungs?
2.13 L
you have a 30.0 L cylinder of helium at a pressure of 132 atm and a temperature of 19 degrees celcius. the He is used to fill balloons to a volume of 1.80 L at 745 mm Hg and 27 degrees celcius. how many balloons can be filled with He? assume that the cylinder can provide He until its internal pressure reaches 1.00 atm (i.e. there are 131 atm of usable He in the cylinder.)
2.29x10^3
a balloon has a volume of 2.37 liters at 24.0 degrees celcius. the balloon is heated to 48.0 degrees celcius. calculate the new volume of the balloon.
2.56 L
which of the following expressions does not represent a proper expression for the rate of this reaction? 2A+3B=F+2G a) (-Δ[A])/(Δt) b) (Δ[F])/(Δt) c) (-Δ[B])/(3Δt) d) (Δ[G])/(2Δt)
a
which of the following is the strongest intermolecular force present in NH3?
hydrogen bonding
According to the Bronsted-Lowry definition, an acid [ ]
is a proton donor.
delta G< 0 for a reaction indicated that [ ].
it is spontaneous
non ideal behavior for a gas is most likely to be observed under conditions of
low temperature and high pressure
review voltaic cell image
on phone
The space-filling representation provided below is an example of a _____ unit cell, which contains 1 atom.
primitive cubic (review pictures)
Given the initial rate data for the reaction A+B=C, determine the rate expression for the reaction. [A], M [B], M delta[C]/delta t (initial) M/s 0.0418. 0.122 2.73 x 10^-4 0.0836. 0.122 10.9 x 10^-4 0.0418. 0.488 2.73 x 10^-4
rate= 0.156M^-1s^-1[A}^2
the thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows. N2(g)+3H2(g)=2NH3(g). deltaH=-92.2 kJ if at equilibrium, which would cause the reaction to proceed to the left?
removing H2(g)
the best explanation for the existence of a meniscus observed when water is placed in a glass tube of small diameter is
the attractive forces between the water molecules and the walls of the container are greater than the attractive forces between the water molecules
if the reaction quotient Q is greater than K in a gas phase reaction, then
the reaction will proceed in the backward direction until equilibrium is established.
the reaction quotient Q for a system is 1.6x10^-4. If the equilibrium constant for the system at some temperature is 8.5x10^3, what will happen as the reaction mixture returns to equilibrium?
there will be a net loss in reactants.
all of the following are colloidal dispersions except: cheese, white wine, milk, whipped cream, marshmallow
white wine
which of the following pure liquids is expected to have the highest boiling point? NO, ICl, PH3, CO, AsH3
ICl
what is the Kc expression for the equilibrium given below? CuBr(s)=Cu^++Br^-(aq)
K=[Cu^+][Br^-]
place the following cations in order of their hydration enthalpy: Li^+, H^+, K^+
K^+<Li^+<H^+
what is the Kc equilibrium constant expression for the following equilibrium? NiO(s)+H2(g)=Ni(s)+H2O(g)
Kc=[H2O]/[H2]
if an ionic solid has a face centered cubic lattice of anions (X^n-) and all the octahedral holes are occupied by metal cations (M^m+), what is the formula for the compound ?
MX
which of the following is the correct equation for the reaction of ammonia and water?
NH3(aq)+H2O(l)=NH4^++OH^-(aq)
As pure molecular solids, which of the following exhibits dipole-dipole intermolecular forces: PH3, SO3, HCl, and CO2?
PH3 and HCl
ammonia (NH3) is used as a refrigerant. at this bp of -33 degrees celcius, the standard enthalpy of vaporization of ammonia is 23.3 kj/mol. how much heat is released when 50.0 g of ammonia is condensed at -33 degrees celcius?
-68.4 kJ
what is the standard entropy change for the following reaction? 4N2(g)+12 H2(g)=8 NH3(g) S^0298 -> 191.5. 130.6. 192.3
-794.8 J/K*mol-rxn
which of the following statements is true for the following reactions, assuming it moves towards products Fe^3+(aq)+Co(s)=Fe^2+(aq)+Co^2+(aq)
Co(s) is oxidized and Fe^3+(aq) is reduced.
for a chemical reaction, the activation energy for the forward reaction is +181 kJ and the activation energy for the backward reaction is +62 kJ. what is the net energy change for the forward reaction?
+119 kJ
what is the freezing point of a 0.27 m solution of glucose, C6H12O6 (MW=180.16 g/mol) in water (Kfp for water is 1.858 degrees celcius/m)
-0.50 degrees celcius
calculate the standard entropy change for the following reaction: 2 SO2(g)+O2(g)=2 SO3(g) given: S[SO2(g)]=248.2 J/K*mol, S[O2(g)]=205.1 J/K*mol, and S[SO3(g)]=256.8 J/K*mol
-187.9 J/K*mol-rxn
calculate delta G of the reaction at 25 degrees celcius for the reaction below: 2 Na(s)+2 H2O(l)=2 NaOH(aq)+H2(g) given: delta H= -366.6 kJ/mol*rxn and delta S=-154.2 J/K*mol*rxn
-320.6 kJ/mol*rxn
write a balanced chemical equation for the following redox reaction occurring in an acidic solution Cr2O7^2-(aq)+Ni(s)=Cr^3+(aq)+Ni^2+(aq)
Cr2O7^2-(aq)+3 Ni(s)+ 14 H^+(aq)=2Cr^3+(aq)+3Ni^2+(aq)+7H2O(l)
which of the following strong electrolytes has the LEAST negative hydration enthalpy? LiBr, RbBr, CsBr, NaBr
CsBr
which of the following nonpolar molecules has the lowest boiling temperature? C5H12 C7H16 C4H10 C8H18 C6H14
C4H10
as pure molecular solids which of the following exhibit only induced dipole/induced dipole forces: CO2, CH2Cl2, and SO2?
CO2 and CH2Cl2
Colloids are described by all of the following except: a. The particles in a colloid are so small that settling is negligible. b. The mixture appears cloudy. c. Only combinations of liquids and gases can form colloids. d. Colloids are not suspensions or homogeneous mixtures. e. Mayonnaise, whipped cream and fog are all examples of colloids.
c
what is the name given to a substance that increases the rate of a chemical reaction but is not itself consumed?
catalyst
which of the following intermolecular forces or bonds is primarily responsible for the solubility of Argon (Ar) in water? ion-induced dipole hydrogen bonding dipole-dipole hydrogen bonding-dipole force dipole-induced dipole
dipole-induced dipole