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engineering
the science and engineering of materials

Questions and Answers of The Science And Engineering Of Materials

Choose the statements that correctly describe the following phase diagram. a. If the temperature is raised from 50 K to 400 K at a pressure of 1 atm, the substance boils at approximately 185
The molar heat of fusion of benzene (C6H6) is 9.92 kJ/mol. Its molar heat of vaporization is 30.7 kJ/mol. Calculate the heat required to melt 8.25 g benzene at its normal melting point. Calculate the
Which is stronger, a dipole–dipole interaction between two molecules or a covalent bond between two atoms within the same molecule? Explain.
Which of the following compound(s) exhibit only London dispersion intermolecular forces? Which compound(s) exhibit hydrogen-bonding forces? Considering only the compounds without hydrogen-bonding
Which of the following statements is(are) true?a. LiF will have a higher vapor pressure at 25οC than H2S.b. HF will have a lower vapor pressure at -50οC than HBr.c. Cl2 will have a higher boiling
Pyrolusite is a mineral containing manganese ions and oxide ions. Its structure can best be described as a body-centered cubic array of manganese ions with two oxide ions inside the unit cell and two
Some ice cubes at 0οC with a total mass of 403 g are placed in a microwave oven and subjected to 750. W (750. J/s) of energy for 5.00 minutes. What is the final temperature of the water? Assume all
The enthalpy of vaporization for acetone is 32.0 kJ/mol. The normal boiling point for acetone is 56.5οC. What is the vapor pressure of acetone at 23.5οC?
When 1 mole of benzene is vaporized at a constant pressure of 1.00 atm and at its boiling point of 353.0 K, 30.79 kJ of energy (heat) is absorbed and the volume change is +28.90 L. What are ΔE and
A 0.132-mole sample of an unknown semiconducting material with the formula XY has a mass of 19.0 g. The element X has an electron configuration of [Kr]5s2 4d10. What is this semiconducting material?
The four most common ways to describe solution composition are mass percent, mole fraction, molarity, and molality. Define each of these solution composition terms. Why is molarity
What does the axiom “like dissolves like” mean? There are four types of solute/solvent combinations: polar solutes in polar solvents, nonpolar solutes in polar solvents, and so on. For each type
Assume that you place a freshwater plant into a saltwater solution and examine it under a microscope. What happens to the plant cells? What if you placed a saltwater plant in pure water? Explain.
How does ΔHsoln relate to deviations from Raoult’s law? Explain.
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: “The solute and solvent can be
You drop an ice cube (made from pure water) into a saltwater solution at 0οC. Explain what happens and why.
What is osmotic pressure? How is osmotic pressure calculated? Molarity units are used in the osmotic pressure equation. When does the molarity of a solution approximately equal the molality of the
You and your friend are each drinking cola from separate 2-L bottles. Both colas are equally carbonated. You are able to drink 1 L of cola, but your friend can drink only about half a liter. You each
Distinguish between a strong electrolyte, a weak electrolyte, and a nonelectrolyte. How can colligative properties be used to distinguish between them? What is the van’t Hoff factor? Why is the
Is molality or molarity dependent on temperature? Explain your answer. Why is molality, and not molarity, used in the equations describing freezing-point depression and boiling-point elevation?
What is a colloidal dispersion? Give some examples of colloids. The Tyndall effect is often used to distinguish between a colloidal suspension and a true solution. Explain. The destruction of a
Consider a beaker of salt water sitting open in a room. Over time, does the vapor pressure increase, decrease, or stay the same? Explain.
If a solution shows positive deviations from Raoult’s law, would you expect the solution to have a higher or lower boiling point than if it were ideal? Explain.
The two beakers in the sealed container illustrated below contain pure water and an aqueous solution of a volatile solute.If the solute is less volatile than water, explain what will happen to the
What mass of sodium oxalate (Na2C2O4) is needed to prepare 0.250 L of a 0.100-M solution?
The following plot shows the vapor pressure of various solutions of components A and B at some temperature.Which of the following statements is false concerning solutions of A and B?a. The solutions
What volume of 0.25 M HCl solution must be diluted to prepare 1.00 L of 0.040 M HCl?
What volume of a 0.580-M solution of CaCl2 contains 1.28 g solute?
The weak electrolyte NH3(g) does not obey Henry’s law. Why? O2(g) obeys Henry’s law in water but not in blood (an aqueous solution). Why?
When pure methanol is mixed with water, the resulting solution feels warm. Would you expect this solution to be ideal? Explain.
Detergent molecules can stabilize the emulsion of oil in water as well as remove dirt from soiled clothes. A typical detergent is sodium dodecylsulfate, or SDS, and it has a formula of
For an acid or a base, when is the normality of a solution equal to the molarity of the solution and when are the two concentration units different?
In order for sodium chloride to dissolve in water, a small amount of energy must be added during solution formation. This is not energetically favorable. Why is NaCl so soluble in water?
Adding a solute to a solvent extends the liquid phase over a larger temperature range. Explain this statement.
Table sugar (C12H22O11) or urea [(NH2)2CO] can be used by road crews to melt ice on roads, but solutions of CaCl2 are generally used instead. Assuming equal costs per pound of substance, why is CaCl2
If two different aqueous solutions of proteins have the same boiling point, what other physical properties are the same between the two solutions? Assume dilute solutions.
An extremely important application of dialysis is the use of artificial kidney machines to purify blood. Explain how dialysis can be used to purify blood.
Explain the terms isotonic solution, crenation, and hemolysis.
Common commercial acids and bases are aqueous solutions with the following properties: Calculate the molarity, molality, and mole fraction of each of the preceding reagents. Hydrochloric
What is ion pairing?
A solution of phosphoric acid was made by dissolving 10.0 g H3PO4 in 100.0 mL water. The resulting volume was 104 mL. Calculate the density, mole fraction, molarity, and molality of the solution.
An aqueous antifreeze solution is 40.0% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.05 g/cm3. Calculate the molality, molarity, and mole fraction of the ethylene glycol.
In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would proceed using the given information. a. 2.0 m KCl in water (density of H2O = 1.00 g/cm3)b.
A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63 g/cm3) with 45 mL hexane (C6H14, d = 0.66 g/cm3). Assuming that the volumes add on mixing, calculate the mass percent, mole fraction,
a. Calculate the freezing-point depression and osmotic pressure at 25οC of an aqueous solution containing 1.0 g/L of a protein (molar mass = 9.0 × 104 g/mol) if the density of the solution is 1.0
A solution is prepared by mixing 50.0 mL toluene (C6H5CH3, d = 0.867 g/cm3 ) with 125 mL benzene (C6H6, d = 0.874 g/cm3). Assuming that the volumes add on mixing, calculate the mass percent, mole
Calculate the molarity and mole fraction of acetone in a 1.00-m solution of acetone (CH3COCH3) in ethanol (C2H5OH). (Density of acetone = 0.788 g/cm3; density of ethanol = 0.789 g/cm3.) Assume that
Calculate the normality of each of the following solutions. a. 0.250 M HClb. 0.105 M H2SO4c. 5.3 × 10-2 M H3PO4d. 0.134 M NaOHe. 0.00521 M Ca(OH)2What is the equivalent mass for each of the
The vapor pressures of several solutions of water–propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45οC:a. Are solutions of water and propanol
The lattice energy* of NaI is -686 kJ/mol, and the enthalpy of hydration is -694 kJ/mol. Calculate the enthalpy of solution per mole of solid NaI. Describe the process to which this enthalpy change
An aqueous solution containing glucose has a vapor pressure of 19.6 torr at 25°C. What would be the vapor pressure of this solution at 45°C? The vapor pressure of pure water is 23.8 torr at 25°C
The normal boiling point of diethyl ether is 34.5οC. A solution containing a nonvolatile solute dissolved in diethyl ether has a vapor pressure of 698 torr at 34.5οC. What is the mole fraction of
A solution is prepared by dissolving 27.0 g urea, (NH2)2CO, in 150.0 g water. Calculate the boiling point of the solution. Urea is a nonelectrolyte.
A 2.00-g sample of a large biomolecule was dissolved in 15.0 g carbon tetrachloride. The boiling point of this solution was determined to be 77.85οC. Calculate the molar mass of the biomolecule. For
What mass of glycerin (C3H8O3), a nonelectrolyte, must be dissolved in 200.0 g water to give a solution with a freezing point of -1.50οC?
What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 15.0 L water to produce an antifreeze solution with a freezing point of -25.0οC? What is the boiling point of this
Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpentina. It was first synthesized in 1956 by Nobel Prize winner R. B. Woodward. It is used as a tranquilizer and
Erythrocytes are red blood cells containing hemoglobin. In a saline solution they shrivel when the salt concentration is high and swell when the salt concentration is low. In a 25οC aqueous solution
An aqueous solution of 10.00 g of catalase, an enzyme found in the liver, has a volume of 1.00 L at 27οC. The solution’s osmotic pressure at 27οC is found to be 0.745 torr. Calculate the molar
A 0.15-g sample of a purified protein is dissolved in water to give 2.0 mL of solution. The osmotic pressure is found to be 18.6 torr at 25οC. Calculate the protein’s molar mass.
How would you prepare 1.0 L of an aqueous solution of sucrose (C12H22O11) having an osmotic pressure of 15 atm at a temperature of 22οC? Sucrose is a nonelectrolyte.
How would you prepare 1.0 L of an aqueous solution of sodium chloride having an osmotic pressure of 15 atm at 22οC? Assume sodium chloride exists as Na+ and Cl- ions in solution.
Use the following data for three aqueous solutions of CaCl2 to calculate the apparent value of the van’t Hoff factor. Molality Freezing-Point Depression (°C) 0.0225 0.0910 0.278 0.110 0.440 1.330
Consider the following solutions:0.010 m Na3PO4 in water0.020 m CaBr2 in water0.020 m KCl in water0.020 m HF in water (HF is a weak acid.)a. Assuming complete dissociation of the soluble salts, which
From the following:pure watersolution of C12H22O11 (m = 0.01) in watersolution of NaCl (m = 0.01) in watersolution of CaCl2 (m = 0.01) in waterChoose the one with the a. Highest freezing
Calculate the freezing point and the boiling point of each of the following aqueous solutions. (Assume complete dissociation.)a. 0.050 m MgCl2b. 0.050 m FeCl3
The freezing-point depression of a 0.091-m solution of CsCl is 0.320οC. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440οC. In which solution does ion association appear to be
A 0.500-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 2.50 atm at 25οC. If each molecule of the solute dissociates into
Would benzoic acid be more or less soluble in a 0.1-M NaOH solution than it is in water?
A 0.25-m aqueous solution of Na3PO4 has a freezing point of –1.6°C. Is this solution behaving ideally?
The term proof is defined as twice the percent by volume of pure ethanol in solution. Thus, a solution that is 95% (by volume) ethanol is 190 proof. What is the molarity of ethanol in a 92 proof
At 25οC, the vapor in equilibrium with a solution containing carbon disulfide and acetonitrile has a total pressure of 263 torr and is 85.5 mole percent carbon disulfide. What is the mole fraction
If the human eye has an osmotic pressure of 8.00 atm at 25οC, what concentration of solute particles in water will provide an isotonic eyedrop solution (a solution with equal osmotic pressure)?
The freezing point of an aqueous solution is -2.79οC.a. Determine the boiling point of this solution.b. Determine the vapor pressure (in mm Hg) of this solution at 25οC (the vapor pressure of
A solution at 50°C containing 2.0 mol of liquid A and 3.0 mol of liquid B has a total vapor pressure of 240. torr. If pure A has a vapor pressure of 150. torr at 50°C, what is the vapor pressure of
The normal boiling point of methanol is 64.7οC. A solution containing a nonvolatile solute dissolved in methanol has a vapor pressure of 556 torr at 64.7οC. What is the mole fraction of methanol in
The molar mass of a nonelectrolyte is 58.0 g/mol. Determine the boiling point of a solution containing 35.0 g of this compound and 600.0 g of water. The barometric pressure during the experiment was
A 4.7 × 10-2 mg sample of a protein is dissolved in water to make 0.25 mL of solution. The osmotic pressure of the solution is 0.56 torr at 25οC. What is the molar mass of the protein?
The vapor pressure of pure benzene is 750.0 torr and the vapor pressure of toluene is 300.0 torr at a certain temperature. You make a solution by pouring “some” benzene with “some” toluene.
Plants that thrive in salt water must have internal solutions (inside the plant cells) that are isotonic with (have the same osmotic pressure as) the surrounding solution. A leaf of a saltwater
You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be -0.426οC. Assuming ideal behavior, calculate the mass
An aqueous solution is 1.00% NaCl by mass and has a density of 1.071 g/cm3 at 25οC. The observed osmotic pressure of this solution is 7.83 atm at 25οC.a. What fraction of the moles of NaCl in
A solid mixture contains MgCl2 and NaCl. When 0.5000 g of this solid is dissolved in enough water to form 1.000 L of solution, the osmotic pressure at 25.0οC is observed to be 0.3950 atm. What is
You have a solution of two volatile liquids, A and B (assume ideal behavior). Pure liquid A has a vapor pressure of 350.0 torr and pure liquid B has a vapor pressure of 100.0 torr at the temperature
Specifications for lactated Ringer’s solution, which is used for intravenous (IV) injections, are as follows to reach 100. mL of solution: 285–315 mg Na+14.1–17.3 mg K+4.9–6.0 mg
Creatinine, C4H7N3O, is a by-product of muscle metabolism, and creatinine levels in the body are known to be a fairly reliable indicator of kidney function. The normal level of creatinine in the
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Consider the following statements: “In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get ‘warmed up.’ After that, however, the
Describe at least two experiments you could perform to determine a rate law.
Make a graph of [A] versus time for zero-, first-, and secondorder reactions. From these graphs, compare successive half lives.
Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the “rate law”? What is k in a rate law, and what are orders in a rate law? Explain.
Derive expressions for the half-life of zero-, first-, and second-order reactions using the integrated rate law for each order. How does each half-life depend on concentration? If the half-life for a
A friend of yours states, “A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equation.” What do you tell your friend?
Provide a conceptual rationale for the differences in the halflives of zero-, first-, and second-order reactions.
What is the premise underlying the collision model? How is the rate affected by each of the following?a. Activation energyb. Temperaturec. Frequency of collisionsd. Orientation of collisionsSketch a
The rate constant (k) depends on which of the following (there may be more than one answer)? a. The concentration of the reactantsb. The nature of the reactantsc. The temperatured. The order of
Each of the statements given below is false. Explain why. a. The activation energy of a reaction depends on the overall energy change (ΔE) for the reaction.b. The rate law for a reaction can be
The type of rate law for a reaction, either the differential rate law or the integrated rate law, is usually determined by which data is easiest to collect. Explain.
The rate of the reaction depends only on the concentration of nitrogen dioxide below 225οC. At a temperature below 225οC, the following data were collected:Determine the rate law, the
Hydrogen reacts explosively with oxygen. However, a mixture of H2 and O2 can exist indefinitely at room temperature. Explain why H2 and O2 do not react under these conditions.

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