Question: The energy available from the world’s

> What is the mass, in g, of 15.0 mol of carbon?

> Calculate the number of mol corresponding to: a. 0.10 g Ca b. 4.00 g Fe c. 2.00 kg N2

> What is the mass, in g, of 1.00 mol of nitrogen atoms?

> How many g of carbon are contained in 3.00 mol of carbon atoms?

> How many mol of sodium correspond to 1.0 × 1015 atoms of sodium?

> How many mercury atoms are present in 1.0 × 10-10 mol of mercury?

> A 4.00-g sample of Fe3O4 reacts with O2 to produce Fe2O3: 4Fe3O4 (s) 1 O2 (g)−−−−→6Fe2O3 (s) Determine the number of g of Fe2O3 produced.

> What is the mass, in g, of Avogadro’s number of iron atoms?

> What is the average molar mass of? a. S b. Na c. Hg

> How many mol of lead (Pb) atoms are equivalent to six billion lead atoms?

> What is the average mass (in amu) of? a. Zr b. Cs c. Ca

> Identify the oxidizing agent, reducing agent, substance oxidized, and substance reduced in the reaction described in Question 4.10. Question 4.10: Write the oxidation half-reaction, the reduction half-reaction, and the complete reaction for the formati

> If the actual yield of oxygen gas in Question 4.114 is 1.10 × 10-2 g, what is the % yield? Question 4.114: Chemical Control of Microbes (Section 4.8) describes the breakdown of the antiseptic H2O2 with the balanced equation 2H2O2(aq) −−−−→ 2H2O(l) + O2

> The reaction of calcium hydride with water can be used to prepare hydrogen gas: CaH2 (s) 1 2H2O(l)−−−→Ca (OH)2 (aq) + 2H2 (g) How many g of hydrogen gas are produced in the reaction of 1.00 × 102 g calcium hydride with water?

> Dinitrogen monoxide (also known as nitrous oxide and used as an anesthetic) can be made by heating ammonium nitrate: NH4NO3 (s) −−D−→ N2O(g) + 2H2O(g) How many g of dinitrogen monoxide can be made from 1.00 3 102 g of ammonium nitrate?

> A 3.5-g sample of water reacts with PCl3 according to the following equation: 3H2O(l) + PCl3 (g)−−−→H3PO3 (aq) + 3HCl(aq) How many mol of H3PO3 are produced?

> How many g of Al will react with 3.00 mol of O2? 4Al(s) + 3O2 (g)−−−→2Al2O3 (s)

> Chemical Control of Microbes (Section 4.8) describes the breakdown of the antiseptic H2O2 with the balanced equation 2H2O2(aq) −−−−→ 2H2O(l) + O2(g). Assuming there is an unlimited amount of the enzyme, how many g of O2 would be produced from 1.00 × 10-1

> Describe the steps used in the calculation of g of product resulting from the reaction of a specified number of g of reactant.

> Write the oxidation half-reaction, the reduction half-reaction, and the complete reaction for the formation of calcium iodide from calcium metal and I2. Remember, the electron gain must equal the electron loss.

> Write the two conversion factors that can be written for the relationship between cm and in.

> The following four measurements were made for an object whose true volume is 17.55 mL. 18.69 mL, 18.69 mL, 18.70 mL, 18.71 mL Describe the measurements in terms of their accuracy and their precision.

> For any given principal energy level, what is the maximum number of electrons that can exist in the following subshells? a. s b. p c. d

> Distinguish between a sublevel and an orbital.

> Use the graph prepared in Question 2.75 to predict the melting point of francium (Fr). Question 2.75: Element Atomic Number Melting Point (C) Li 3 180.5 Na 11 97.8 K 19 63.3 Rb 37 38.9 Cs 55 28.4

> Which group of the periodic table is known as the alkaline earth metals? List their symbols.

> What English unit of volume is similar to a L?

> What was the major deficiency of Bohr’s atomic model?

> What is the relationship between density and specific gravity?

> Give two reasons why the Bohr theory did not stand the test of time.

> Assume the Body-Mass Index (BMI) is calculated using the expression BMI = weight (kg)/height2 (m2). If a patient has a height of 1.6 m and a BMI of 38 kg/m2, what is the patient’s weight in both kg and lb?

> Critique this statement: Promotion of electrons is accompanied by a release of energy.

> The density of mercury is 13.6 g/mL. If a sample of mercury weighs 272 g, what is the volume of the sample in mL?

> When electrical energy is applied to an element in its gaseous state, light is produced. How does the light differ among elements?

> The specific gravity of a patient’s urine sample was measured to be 1.008. Given that the density of water is 1.000 g/mL at 40C, what is the density of the urine sample?

> What is the relationship between the energy of light and its wavelength?

> The density of methanol at 200C is 0.791 g/mL. What is the mass of a 50.0 mL sample of methanol?

> Describe electromagnetic radiation according to its particle nature.

> Refer to Question 1.129. Suppose that each of the bars had the same mass. How could you determine which bar had the lowest density and which had the highest density? Question 1.129: You are given three bars of metal. Each is labeled with its identity (

> Predict the polarity of each compound in Question 3.98. Question 3.98: a. SeO2 b. SeO3

> You are given a piece of wood that is either maple, teak, or oak. The piece of wood has a volume of 1.00 × 102 cm3 and a mass of 98 g. The densities of maple, teak, and oak are as follows: What is the identity of the piece of wood? Woo

> K+ and Ar are isoelectronic. Which is larger? Why?

> What is meant by the term electromagnetic spectrum?

> What is the mass of a femur (leg bone) having a volume of 118 cm3? The density of bone is 1.8 g/cm3.

> Draw a diagram representing a homogeneous mixture of two different substances. Use two different colored spheres to represent the two different substances.

> Arrange each of the following lists of elements in order of decreasing electron affinity: a. Mg, P, Cl b. Br, I, Cl

> Calculate the density of 50.0 g of an isopropyl alcohol– water mixture (commercial rubbing alcohol) that has a volume of 63.6 mL.

> Arrange each of the following lists of elements in order of increasing ionization energy: a. Cl, Br, I b. Ra, Be, Mg

> Write the electron configuration and shorthand electron configuration of each of the following biologically important ions: a. Ca2+ b. Mg2+ c. K+ d. Cl-

> A physiological solution designed to replace a patient’s lost K+ is 40 meq/L in K+ and 40 meq/L in Cl-. a. Calculate the number of mol of K+ in 1.00L of solution. b. Calculate the number of mol of Cl- in 1.00L of solution.

> Which of the following pairs of atoms and/or ions are isoelectronic with one another? a. F-, Cl- b. K+, Ar

> Write an equation for the addition of an electron to a gaseous atom of chlorine.

> The weather station posted that the low for the day would be -100F. Convert -10.00F to: a. 0C b. K

> Define electron affinity.

> Give the most probable ion formed from each of the following elements. a. O b. Br c. Al

> If the potassium ion concentration in the solution described in Question 6.113 was only 35 meq/L, calculate the potassium ion concentration in units of mol/L. Question 6.113: A potassium chloride solution that also contains 5% (m/V) dextrose is adminis

> Label each of the following statements as true or false. If false, correct the statement. a. Energy can be created or destroyed. b. Energy can be converted from electrical energy to light energy. c. Conversion of energy from one form to another can occur

> Why is the melting point of silicon much higher than that of argon, even though argon has a greater molar mass?

> Rank the following temperatures from coldest to hottest: zero degrees Celsius, zero degrees Fahrenheit, zero Kelvin

> Calculate the number of eq/L of SO42- in a solution that is 2.5 × 10-3 M in SO42-.

> Explain why a dialysis solution must have an elevated potassium ion concentration when loss of potassium ions from the blood is a concern.

> The sequence of a gene on the mRNA is normally AUGCCCGACUUU. A point mutation in the gene results in the mRNA sequence AUGCCGGACUUU. What are the amino acid sequences of the normal and mutant proteins? Would you expect this to be a silent mutation?

> Predict the number of valence electrons in an atom of: a. carbon b. phosphorus c. sulfur d. chlorine

> The pH of blood plasma from a patient was found to be 7.6, a life-threatening situation. Calculate the ratio [HCO3-]/[H2CO3] in this sample of blood plasma. (Ka of H2CO3, carbonic acid, is 4.5 × 10-7.)

> Which volume is smaller: 1.0 L or 1.0 qt?

> Highly substituted alkyl fluorides, called perfluoroalkanes, are often used as artificial blood substitutes. These perfluoroalkanes have the ability to transport O2 through the bloodstream as blood does. Some even have twice the O2 transport capability a

> Which volume is smaller: 50.0 mL or 0.500 L?

> What is the function of unsaturation in the hydrocarbon tails of membrane lipids?

> A newborn is 21 in in length and weighs 6 lb 9 oz. Describe the baby in metric units.

> List the enzymes whose levels are elevated as a result of hepatitis or cirrhosis of the liver.

> If a drop of blood has a volume of 0.05 mL, how many drops of blood are in the adult described in Question 1.99? Question 1.99: A 150 lb adult has approximately 9 pt of blood. How many L of blood does the individual have?

> What are the nine essential amino acids?

> Noble gases in the third period and beyond can undergo covalent bonding. All have an expanded octet. Draw the Lewis structure of XeF2.

> Use the concept of charges to explain why an alpha particle fired toward the nucleus is deflected away from the nucleus.

> How are citric acid cycle intermediates replenished when they are in demand for biosynthesis?

> Convert 7.5 × 10-3 cm to mm.

> What amino acids are synthesized from a-ketoglutarate?

> Use the concept of charges to explain why cathode rays are specifically deflected toward the positive pole by external electric fields and magnetic fields.

> Three ATP are hydrolyzed to provide the energy for the urea cycle.

> Convert 5.0 qt to: a. gal b. pt c. L d. mL e. µL

> How does glucagon affect lipid metabolism?

> Distinguish between an intensive property and an extensive property.

> How does glucagon affect carbohydrate metabolism?

> Triglycerides (Chapters 17 and 23) are used in biochemical systems to store energy; they can be formed from glycerol and fatty acids. The molecular formula of glycerol isC3H8O3. Calculate: a. the formula mass of glycerol b. the number of oxygen atoms in

> Describe what is meant by an extensive property and give an example.

> Where is glucagon produced?

> Why is it important to always include units when recording measurements?

> What are the primary target cells of glucagon?

> Give examples of pure substances and mixtures.

> What are the primary target cells of insulin?

> Express each of the following numbers in standard notation: a. 3.24 × 103 b. 1.50 × 104 c. 4.579 × 10-1 d. -6.83 × 105 e. -8.21 3× 10-2 f. 2.9979× 108 g. 1.50 × 100 h. 6.02 × 1023

> What is the trigger that causes insulin to be secreted into the bloodstream?

> Perform each of the following operations, reporting the answer with the proper number of significant figures: (16.0)(0.1879) а. d. 18 + 52.1 45.3 (76.32)(1.53) b. e. 58.17 – 57.79 0.052 (0.0063)(57.8) с.

> What is the source of the glycerol molecule that is used in the synthesis of triglycerides?

> Sally and Gertrude were comparing their weight-loss regimens. Sally started her diet weighing 193 lb. In 1 year she weighed 145 lb. Gertrude started her diet weighing 80 kg. At the end of the year, she weighed 65 kg. Who lost the most weight? a. Describe

> Round the following numbers to three significant figures: a. 123700 b. 0.00285792 c. 1.421 × 10-3 d. 53.2995 e. 16.96 f. 507.5

> Why can’t the brain use fatty acids as fuel?

> How many significant figures are represented in each of the following numbers? a. 3.8 × 10-3 b. 5.20 × 102 c. 0.00261 d. 24 e. 240 f. 2.40

> How are triglyceride synthesis and degradation regulated in adipose tissue?

> Explain what is meant by each of the following terms: a. error b. uncertainty