Exam 1
You have equal mass percent concentrations of the following solutions. Which of the following would you expect to have the highest molality.
A: NaCl
B:NaF
C: LiCl
D:LiF
E: KCl
D: LiF
Consider the following equilibrium
C(s)+CO2(g)-><- 2CO(g) Delta H= +172.5kJ
Which of the following would result in an equilibrium shift to the right?
A: Lowering the temperature
B: Increase in Pressure
C: Increase in volume
D: Adding C Solid
E: Adding a catalyst
A: Lowering the temperature
In a solution of CaF2, the [Ca^2+] and the [F-} are equal. Also, Q is less than the Ksp value. This means
A: Only more Ca2+ can be dissolved
B: Only more F- can be dissolved
C: Both more Ca2+ and F- can be dissolved
D: Neither Ca2+ nor F- can be dissolved
E: Not enough infomation given
C: Both more Ca2+ and F- can be dissolved
Suppose 1 mole of sugar dissolves into 4 moles water. The vapor pressure of the resulting solution would be
A: 90% of the vapor pressure of water
B: 80% of the vapor pressure of water
C: 75% of the vapor pressure of water
D: 25% of the vapor pressure of water
E: 20% of the vapor pressure of water
B: 80% of the vapor pressure of water
For a ceratin reaction the standard free energy change is +60kJ at -100C and +30kJ at -50C. For this raction
A: Delta H Knot is positive and Delta S Knot is postive.
B: Delta H Knot is Negative and Delta S Knot is Negative
C: Delta H Knot is negative and Delta S Knot is postive
D: Delta H Knot is positive and Delta S Knot is negative.
E: More information is needed
A: Delta H Knot is positive and Delta S Knot is postive.
Suppose a first order kinetic reaction has a half-life of 4 minutes. How much of the original compound would be left after 8 minutes?
A: 3/4
B: 1/2
C: 1/4
D: 1/8
E: None of the compound would be left
C: 1/4
The cation of a weak base
A: Is a basic ion
B: Is an acidic ion
C: Is a neutral ion
D: Will increase the pH of the solution
E: Will produce OH- ions in water
E: Will produce OH- ions in water
This reaction would be
A: Spontaneous at high temperature, not spontaneous at low temperature
B: Spontaneous at low temperature, not spontaeous at high temperature
C: Spontanrous at all temperatures
D: Not spontaneous at any temperatures
E: Need to know the actual temperatures to answer
B: Spontaneous at low temperature, not spontaeous at high temperature
A salt has the formula MX in which M is a metal ion and X is an anion. Which of the following will make MX a neutral salt?
A: M is the cation of a strong base and X is the anion of a strong acid.
B : M is the cation of a weak base and X id the anion of a strong acid.
C: M is the cation of a strong base and X is the anion of a weak acid
D: M is the cation of a weak base and X is the anion of a weak acid
E: None of the above.
A: M is the cation of a strong base and X is the anion of a strong acid.
Consider a reaction with a standard potential of Eocell. If the concentrations of the reactants are increased, then
A: Eocell will decrease
B: Ecell will decrease
C: Eocell will increase
D: Ecell will increase
E: Eocell and Ecell will remain the same
D: Ecell will increase
The reaction A->B is found to be second order. This means a straight line will be generated from a plot of
A: [A] versus time
B: [A]^2 versus time
C: ln[A] versus time
D: 1/[A] versus time
E: ln[A] versus ln(time)
D: 1/[A] versus time
Consider the following equilibrium expressions
aA(g)+bB(g)-><- cC9g)+dD(g)
at 25C if Kc<Kp this means
A: a+b>c+d
B: c+d>a+b
C: a-b>c-d
D: c-d>a-b
E: a+b=c+d
B: c+d>a+b
Which of the following would NOT be more soluble in acid solution?
A: Ag2SO4
B:CuCO3
C: ZnS
D: AgBr
E: MgF2
D: AgBr
Which of the following will have both a conjugate acid and conjugate base
A: PO4^3-
B: HCO3-
C: S^2-
D: CN-
E: SO3^2-
B: HCO3-
Which of the following, when mixed, would NOT result in a buffer solution?
A: 10mL of .1M HNO2, and 20mL of .1MNaNO2
B: 10mL of .1M HCN, and 10mL of .1M KCN
C: 10mL of .1M NaOH and 20mL of .1M HC2H3O2
D: 10mL of .1M NaOH and 20mL of .1M HF
E: 10mL of .1M HCl and 10mL of .1M NH3
E: 10mL of .1M HCl and 10mL of .1M NH3
Consider the followuing 3-Step mechanism to yield an overall reaction
Step1: A2->2A slow
Step 2: A+B2->AB+B Fast
Step 3: A+B-> AB Fast
Which of the following is a reasonable rate equation?
A: rate=k[A2][B2]
B: rate=k[A2]
C: Rate=k[A]^2
D: Rate=k[A][B2]
E: k[A][B]
B: rate=k[A2]
Consider the following equilibrium reaction
CO2(g)+2H2(g)-><- Ch3OH (g) delta Hknot= -90.8
Which of the following will increase the equilibrium constant, K?
A: Increase in temperature
B: Decrease in temperature
C: Increase in Pressure
D: Decrease in pressure
E: Increase in amount of CH3OH (g)
B: Decrease in temperature
Consider the following cell diagram
Mn(s)/Mn^2+ (1M)//Cr^3+(1M)/Cr(s)
What reaction would be taking place at the cathode?
A: Cr3+ + 3e- -> Cr
B: Mn2+ + 2e- -> Mn
C: Cr-> Cr3+ + 3e-
D: Mn-> Mn2+ + 2e-
E: 3Mn2++2Cr-> 3Mn+2Cr3+
A: Cr3+ + 3e- -> Cr
For a certain equilibrium reaction K=[A][B]/[C]. If the concentrations of A, B, and C are all equal this means
A: K=1
B: K>1
C: K<1
D: K of forward reaction is equal to K of reverse reaction
E: K can't be determined with the infomation given
A: K=1
If the following half reaction is to be used in a cell
2Br-(aq)-> Br2(l)+2e-
Which reaction is an appropriate half reaction to use with this in a functioning electrolytic cell.
A: Au(s)->Au3+(aq)+2e-
B: MnO2(s)+ 4H+(aq)+2e- -> Mn2+(aq)+2H2O(l)
C: Al(s)->Al3+ +3e-
D: I2(g)+2e- -> 2I-(aq)
E: 2Hg2+(aq)+2e- -> Hg2^2+(aq)
B: MnO2(s)+ 4H+(aq)+2e- -> Mn2+(aq)+2H2O(l)
A certain compound is hard, brittle, and high melting. It's a poor conductor; but the melt is a good conductor. This compound is...
A: Ionic
B: Network Covalent
C: Molecular
D: Metallic
E: Amorphous
A: Ionic
Consider the following equilibrium expressions.
A(g)+B(g)-><- C(g)+D(g) with equilibrium constant K1
C(g)+D(g)-><- E(g)+F(g) with equilibrium constant K2
What is the equilibrium constant, K3, for A(g)+B(g)-><- E(g)+F(g)
A: K3=K1+K2
B: K3=K1xK2
C: K3= K1/K2
D: K3=K2/K1
E: K3=K1-K2
B: K3=K1xK2
For the weak acid euilibrium
HA(aq)-><- H+(aq)+A-(aq)
A buffer is made containing HA and A-. If the [HA] is twice the [A-], what is the value of the pH
A. pH is double the pKa
B: pH is 1/2 the value of the pKa.
C: pH is .30 units greate than pKa
D: pH is .30 units less than pKa
E: pH is 1/2 unit greater than pKa
D: pH is .30 units less than pKa
There are two solutions of a weak acid, HA. Solution 1 has a lower pH than solution 2. Which of the following is a true statement?
A: Solution 1 has a higher % ionization and a higher concentration of H+ than Solution 2
B: Solution 1 has a lower % ionization and a lower concentraion of H+ than Solution 2
C: Solution 1 has a higher % ionization and a lower concentration of H+ than Solution 2
D: Solution 1 has a lower % ionization and a higher concentration of H+ than Solution 2
E: Solution 1 and Solution 2 have equal % ionizations and concentraions of H+
A: Solution 1 has a higher % ionization and a higher concentration of H+ than Solution 2