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> Write a balanced nuclear equation for alpha decay of bismuth-212.

> Element 109 was synthesized by bombarding bismuth-209 with iron-58. Write the equation for this process if one product is a neutron.

> Complete the following nuclear equation: ? −−−→ (90 ^ 214) Th + (2 ^4) HE

> Complete the following nuclear equation: (78 ^ 190) Pt −−−→ a + ?

> a. Write the sequence of steps that would be followed for one round of b-oxidation of hexanoic acid. b. Calculate the number of ATP molecules produced by complete b-oxidation of hexanoic acid.

> Complete the following nuclear equation: (92 ^ 238) U + (7 ^14) N−−−−→?6(0 ^1) n

> Write a nuclear equation to represent radium-226 decaying to radon-222 plus an alpha particle.

> Samarium-147 is one of many rare earth isotopes that undergo alpha decay. Write a balanced nuclear equation for this process.

> How many protons and neutrons are contained in each of the three isotopes of carbon?

> How many protons and neutrons are contained in the nucleus of uranium-235?

> Write the nuclear symbol for carbon-14.

> Rank the four major types of radiation in order of size, speed, and penetrating power.

> What is the major difference between beta and gamma radiation?

> Write the nuclear symbol for a beta particle.

> We can control the rate of chemical reactions. Can we control the rate of natural radiation?

> Observed increases in global temperatures are caused by elevated levels of carbon dioxide. Is this statement a theory or a scientific law? Explain your reasoning.

> What are the major differences between alpha particles and gamma radiation?

> What is the composition of a positron?

> What is alpha decay?

> How does the energy of gamma radiation compare with that of other regions of the electromagnetic spectrum?

> A buffer solution is prepared in such a way that the concentration of propanoic acid is 2.00 3 1021 M and the concentration of sodium propanoate is 4.00 3 1021 M. If the buffer equilibrium is described by Ka = 1.34 × 10-5 use the Henderso

> Barium-131 is a radioisotope used to study bone formation. A patient ingested barium-131. How much time will elapse until only one-fourth of the barium-131 remains, assuming that none of the isotope is eliminated from the body through normal processes? T

> Calculate the pH of a buffer system containing 1.0 M NH3 and 1.0 M NH4Cl. (Ka of NH4+, the acid in this system, is 5.6 × 10-10.)

> What is the pH of the solution described in Question 8.101? Question 8.101: What is [H3O+] for a buffer solution that is 0.200 M in acid and 0.500 M in the corresponding salt if the weak acid Ka = 5.80 × 10-7?

> What is meant by the term lethal dose of radiation?

> The half-life of strontium-87 is 2.8 h. What percentage of this isotope will remain after 8 h and 24 minutes (min)?

> What are the roles of DNA, RNA, and protein in information flow in biological systems?

> Write the equilibrium constant expression for the reaction described in Question 7.96. Question 7.96: N2 (g) + O2 (g)↽−−−−⇀2NO(g)

> Will an increase in pressure increase, decrease, or have no effect on the concentration of NO(g) in the reaction: N2 (g) + O2 (g)↽−−−−⇀2NO(g)

> Which of the following are capable of forming a buffer solution? a. HBr and MgCl2 b. H2CO3 and NaHCO3

> Write out each step of the dissociation of chromic acid, H2CrO4.

> Use the equilibrium constant expression you wrote in Question 7.87 and the equilibrium constant you calculated in Question 7.88 to determine the equilibrium concentration of H2S if: Question 7.87: Write the equilibrium constant expression for the react

> Using the equilibrium constant expression in Question 7.87, calculate the equilibrium constant if: Question 7.87: Write the equilibrium constant expression for the reaction: 2H2 (g) 1 S2 (g)↽−−&a

> Chromic acid, H2CrO4, is a polyprotic acid. How many protons can it donate?

> Rewrite the equation in Question 8.82 as a net, balanced ionic equation. Question 8.82: Write an equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of KOH.

> Write an equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of KOH.

> What are the products of a neutralization reaction?

> Calculate formula mass and the molar mass of each of the following formula units: a. S8 b. (NH4)2SO4 c. CO2

> Two nitrogen atoms in a nitrogen molecule are held together more strongly than the two chlorine atoms in a chlorine molecule. Explain this fact by comparing their respective Lewis structures.

> The hydroxide ion concentration in a sample of urine was determined to be of 1.0 × 10-8 M (at 250C). Calculate the hydronium ion concentration of this aqueous solution.

> In a neutralization reaction, how many mol of NaOH are needed to react with 3 mol of HCl?

> Calculate the pH of a solution that has [OH-] = 6.7 × 10-9 M.

> Calculate the pH of a solution that has [H3O+] = 6.6 × 10-5 M.

> Distinguish between the rate constant and the equilibrium constant for a reaction.

> Can a dilute solution of a strong acid ever have a higher pH than a more concentrated solution of a weak acid? Why or why not?

> Write the rate law for the reaction: H2S(aq) + Cl2 (aq)↽−−−−⇀S(s) + 2HCl(aq) Represent the order as n, n', and so forth.

> A 6.00-mL portion of an 8.00 M stock solution is to be diluted to 0.400 M. What will be the final volume after dilution?

> A 50.0-mL sample of a 0.250 M sucrose solution was diluted to 5.00 × 102 mL. What is the molar concentration of the resulting solution?

> Identify the conjugate acid-base pairs for the reversible reactions in Question 8.4. Question 8.4: Write an equation for the reversible reactions of each of the following with water. a. H3PO4 b. CH3NH2

> Calculate [H3O+] for a solution of hydrochloric acid for which: a. pH = 2.00 b. pH = 3.00

> How many g of sodium hydroxide are present in 675 mL of a 0.500 M solution?

> Select one enzyme from a later chapter in this book and describe its biochemical importance.

> What is the concentration of hydronium ions in an aqueous solution of acetaminophen if the concentration of hydroxide ions is 2.5 × 10-9 M?

> Calculate the [OH-] of an aqueous solution that is: a. 1.0 × 10-6 M in H3O+ b. 1.0 × 10-8 M in H3O+

> Calculate the [H3O+] of an aqueous solution that is: a. 1.0 × 10-9 M in OH- b. 1.0 × 10-5 M in OH-

> Label each of the following as a strong or weak base: a. KOH b. CN- c. SO42-

> Of the following diagrams, which one represents: a. a concentrated strong acid b. a dilute strong acid c. a concentrated weak acid d. a dilute weak acid H+ x- H+ x- X- H+ x- H+ H+ x- H+ x- X- H+ x- H+ H+x-H+x=x¯H+ H+ H-X X- Н-X H-X H-X Н-X H-X H-X X

> Identify the conjugate acid-base pairs in each of the following chemical equations: a. HCOOH (aq) + NH3(aq) ↽−−−−−−⇀ HCOO-(aq) + NH4+(aq) b. HCl(aq) + OH-(aq) ↽−−−−−−⇀ H2O(l) + Cl-(aq)

> Which is the stronger base, F2 or CH3COO-?

> Distinguish between the term’s formula mass and molar mass.

> Write an equation for the reversible reactions of each of the following with water. a. H3PO4 b. CH3NH2

> Which is the stronger acid, HNO3 or HCN?

> Write the formula of the conjugate acid of F-.

> Write the formula of the conjugate base of HCOOH.

> Write the formula of the conjugate acid of Br-.

> Write an equation for the reaction of each of the following with water: a. HNO3 b. HCOOH c. CH3CH2CH2NH2

> Classify each of the following as either a Brønsted-Lowry acid, base, or as amphiprotic. a. H2SO4 b. HSO4- c. SO42-

> Classify each of the following as either a Brønsted-Lowry acid, base, or as amphiprotic. a. NH4+ b. NH3 c. CH3CH2CH2NH3+

> Why is ammonia described as a Brønsted-Lowry base and not an Arrhenius base?

> a. Define a base according to the Arrhenius theory. b. Define a base according to the Brønsted-Lowry theory.

> Describe the reaction catalyzed by each of the enzymes listed in Question 22.37. Question 22.37: Match each of the following enzymes with the class of enzyme to which it belongs. (Hint: An enzyme classification may be used more than once or not at all.

> State the second law of thermodynamics.

> Classify each of the following compounds as a Brønsted-Lowry acid or base. a. PO43- b. CH3NH3- c. HI d. H3PO4

> At a given temperature, the equilibrium constant for a certain reaction is 1 × 10-18. Does this equilibrium favor products or reactants? Why?

> Does the attainment of equilibrium imply that no further change is taking place in the system?

> Use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution in which the acetic acid concentration is 2.0 × 10-1 M and the sodium acetate concentration is 1.0 × 10-1 M. The equilibrium constant, Ka, for acetic acid is 1.8 × 10-5.

> For the buffer system described in Question 8.99, which substance is responsible for buffering capacity against added sodium hydroxide? Explain. Question 8.99: For the equilibrium situation involving acetic acid, CH3COOH (aq) + H2O(l) −↽−−−−−−⇀− CH3COO

> True or false: The position of the equilibrium for an endothermic reaction will shift to the right when the reaction mixture is heated. Explain your reasoning.

> Calculate the [OH-] of a solution of hydrochloric acid with pH = 4.00.

> Sketch the interaction of water with an ethanol, CH3CH2OH, molecule.

> Sketch the “interactive network” of water molecules in the liquid state.

> Predict whether each of the following processes increases or decreases entropy, and explain your reasoning. a. burning a log in a fireplace b. condensing of water vapor on a cold surface

> Using the equilibrium constant expression in Question 7.85, calculate the equilibrium constant if: Question 7.85: Write the equilibrium constant expression for the reaction: N2 (g) + 3H2 (g)↽−−&a

> Write a valid equilibrium constant expression for the reaction shown in Question 7.64. Question 7.64: H,S(aq) + Cl2 (aq) =S(s) + 2HCI(aq)

> A change in pressure could have the greatest effect on which type of equilibria: gaseous, liquid, or solid?

> Can a catalyst alter the position of the equilibrium?

> Using the conversion factor in Chapter 1, convert the energy absorbed in Example 7.4 to joules (J). Example 7.4: 7.0 × 102 cal (or 0.70 kcal) of heat energy were absorbed by the dissolution process because the solution lost 7.0 × 102 cal of heat energy

> What is the relationship between the forward and reverse rates for a reaction at equilibrium?

> Calculate the pressure (atm) exerted by 1.00 mol of gas contained in a 7.55-L cylinder at 450C.

> Calculate the density of carbon dioxide at STP.

> Does a large equilibrium constant mean that the reaction must be rapid?

> Explain, in terms of solution properties, why a wilted plant regains its “health” when watered.

> Explain the mechanism by which a fatty acyl group is brought into the mitochondrial matrix

> Calculate the molar volume of O2 gas at STP.

> Predict whether a reaction with positive H and positive S will be spontaneous, nonspontaneous, or temperature dependent. Explain your reasoning.

> Explain how a catalyst can be involved in a chemical reaction without being consumed in the process.

> Distinguish between the terms kinetics and thermodynamics.

> Define and explain the term activation energy as it applies to chemical reactions.

> Provide an example of a reaction that is extremely fast, perhaps quicker than the eye can perceive.

> Which solution is more concentrated: a 20 ppt solution or a 200-ppm solution?