Chem 2 Final.

Hydrogen usually has an oxidation number of

+1

Group 1A and 2A

+1, +2, & F= -1

Oxygen usually has an oxidation number of

-2

The oxidation number of atoms in the uncombined element is...

0

Determine the [OH-] concentration in a 0.169 M Ca(OH)2 solution.

0338 M

List 4 strong acids.

1) H2SO4 2) HCl 3)HBr 4) HNO3

List 4 strong bases.

1) NaOH 2) KOH 3) Ca(OH)2 4) LiOH

What are the units of k in the following rate law? Rate= k[X]^2 [Y]

1/M^2 s

What is the overall order of the following reaction, given the rate law? NO(g)+O3(g)---> NO2(g)+O2(g) Rate= k[NO][O3]

2nd order

What is an amphoteric substance?

A substance that can act as both an acid and a base.

Which of the following is true? A) A buffer resists pH change by neutralizing added acids & bases. B) A buffer does not change pH when strong acid or base is added. C) A buffer is an aqueous solution composed of two weak acids. D) A buffer can absorb an unlimited amount of acid. E) None of the above are true.

A) A buffer resists pH change by neutralizing added acids & bases.

Which of the following processes has a S>0? A) CH4(g)+H2O(g)-->CO(g)+3H2(g) B) CH3OH(l)-->CH3OH(s) C) N2(g)+3H2(g)-->2NH3(g) D) Na2CO3(s)+H2O(g)+CO2(g)-->2NaHCO3(s) E) All of the above processes have a S>0.

A) CH4(g)+H2O(g)-->CO(g)+3H2(g)

Consider a reaction that has a positive H and a positive S. Which of the following statements is true? A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. C) This reaction will be non-spontaneous at all temperatures. D) This reaction will be non-spontaneous only at high temperatures. E) Is is not possible to determine without more information.

A) This reaction will be spontaneous only at high temperatures.

Oxidizing agent

Accepts electrons and becomes reduced.

Which of the following is true? A) A basic solution does not contain H3O+ B) An acidic solution has [H3O+]>[OH-] C) A neutral solution contains [H2O]=[H3O+] D) A neutral solution does not contain any H3O+ or OH- E) None of the above are true

B) An acidic solution has [H3O+]>[OH-]

Identify the triprotic acid. A) HClO4 B) H3PO4 C) H2SO4 D) H2SO3 E) HNO3

B) H3PO4

Identify the process that is spontaneous. A) Frying an egg B) Rusting of iron C) Electrolysis D) Photosynthesis E) Browning of bread

B) Rusting of iron

Consider a reaction that has a negative H and a positive S. Which of the following statements is true? A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. C) This reaction will be non-spontaneous at all temperatures. D) This reaction will be non-spontaneous only at high temperatures. E) Is is not possible to determine without more information.

B) This reaction will be spontaneous at all temperatures.

Which of the following processes shows a decrease in entropy of the system? A) CH3OH(l)-->CO(g)+2H2(g) B) COCl2(g)-->CO(g)+Cl2(g) C) 2NO(g)+O2(g)-->2NO2(g) D) NaClO3(s)-->Na+(aq)+ClO3-(aq) E) None of the above will show a decrease in entropy

C) 2NO(g)+O2(g)-->2NO2(g)

Which of the following is a Bronsted-Lowry base? A) CH4 B) Cl2 C) HCN D) NH3 E) None of the above are Bronsted-Lowry bases.

D) NH3

Which of the following is an Arrhenius base? A) CH3Cl B) LiCl C) CH3CO2H D) NaOH E) More than one of these compounds is an Arrhenius base

D) NaOH

Consider a reaction that has a negative H and a negative S. Which of the following statements is true? A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. C) This reaction will be non-spontaneous at all temperatures. D) This reaction will be non-spontaneous only at high temperatures. E) Is is not possible to determine without more information.

D) This reaction will be non-spontaneous only at high temperatures.

Reducing agent

Donates electrons and becomes oxidized.

The sum of all oxidation numbers of a molecule or ion is...

Equal to its net charge.

What is the overall reaction order for the reaction that has the rate law: Rate= k[F2]^2 [NO]?

First order

Reduction

Gain of electrons

What data should be plotted to show that experimental concentration data fits a first-order reaction?

In [reactant] vs. time

Express the equilibrium constant for the following reaction. CH4(g)+2O2(g)-->CO2(g)+2H2O

K= [CO2][H2O]^2/[CH4][O2]^2

Express the equilibrium constant for the following reaction. 12NH3(g)-->6N2(g)+18H2(g)

K= [N2]^6 [H2]^18/[NH3]^12

Oxidation

Loss of electrons

Give the equation for an unsaturated solution in comparing Q with Ksp.

Q<Ksp

Give the equation for a supersaturated solution in comparing Q with Ksp.

Q>Ksp

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. 2NO(g)+Cl2(g)-->2NOCl

Rate= +1/2 [NOCl]/t

Given the following balanced equation, determine the rate of reaction with respect in [SO2]. 2SO2(g)+O2(g)-->2SO3(g)

Rate= -1/2 [SO2]/Dt

Given the following balanced equation, determine the rate of reaction with respect to [N2]. N2(g)+2H2-->2NH3(g)

Rate= -[N2]/t

Which rate law is unimolecular?

Rate= k[A]

The _______ Law of Thermodynamics states that for any spontaneous reaction, the entropy of the universe increases.

Second

Give the direction of the reaction, if K>>1.

The forward reaction is favored.

Consider the following reaction at equilibrium. What effect will adding more H2S have on the system? 2H2S(g)+3O2-->2H2O(g)+2SO2(g)

The reaction will shift in the direction of products.

Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system? SO2(g)+NO2(g)-->SO3(g)+NO(g)

The reaction will shift in the direction of reactants.

Consider the following reaction at equilibrium. What effect will adding more H2S have on the system? C3H8(g)+5O2(g)-->3CO2(g)+4H2O(l) H=-2220kJ

The reaction will shift to the left in the direction of reactants.

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H2S(g)+3O2(g)-->2H2O(g)+2SO2(g)

The reaction will shift to the right in the direction of products.

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe3O4(s)+CO(g)-->3FeO(s)+CO2 H=+35.9kJ

The reaction will shift to the right in the direction of products.

Give the direction of the reaction, K<<1.

The reverse reaction is favored.

The _____ Law of Thermodynamics states the entropy of a perfect crystal at absolute zero is zero.

Third

Chemical reactions to produce a current are called...

Voltaic & Galvanic cells

A Lewis base

donates an electron pair.

Express the equilibrium constant for the following reaction. Pb(NO3)2(aq)+2NaI(aq)-->PbI2(s)+2NaNO3(aq)

k= [NaNO3]^2/[Pb(NO3)2][NaI]^2

When titrating a strong monoprotic acid and KOH at 25C, the

pH will be equal to 7 at the equivalence point

When titrating a weak monoprotic acid with NaOH at 25C, the

pH will be greater than 7 at the equivalence point.

When titrating a monoprotic strong acid with a weak base at 25C, the

pH will be less than 7 at the equivalence point.

When titrating a weak base with HCl at 25C, the

pH will be less than 7 at the equivalence point.

Which rate law is bimolecular?

rate= k[A][B]

Which rate law is termolecular?

rate= k[A][B]^3

Identify the rate-determining step.

slowest step

The most electronegative element in a compound

takes its lowest oxidation number (which is its group number minus 8)