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chemistry principles and practice

Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions

Scientists have studied the decomposition of hydrogen iodide since the beginning of the 20th century. Some hydrogen iodide was placed in a reactor, which was then heated to 322 °C. The reaction was initiated with 1.25 atm hydrogen iodide; after equilibrium was attained, the partial pressure of HI
Chemists studied the formation of phosgene, COCl2, by sealing 0.96 atm carbon monoxide and 1.02 atm Cl2 in a reactor at 682 K. The pressure declined smoothly from a total pressure of 1.98 atm to 1.22 atm as the system reached equilibrium. Calculate Kp for the following reaction: CO(g) + Cl(g)
A 5.0-L reaction flask initially contains 0.030 mol sulfuryl chloride at 177 °C. Sulfur dioxide and chlorine form:After equilibrium is established, chemical analysis shows that 0.0010 mol sulfuryl chloride remains.(a) Calculate the concentrations of all species.(b) Calculate Kc. SOCl(g) SO(g) +
A 20.0-L container initially contains 2.00 mol NO2, which reacts to form some dinitrogen tetroxide.At equilibrium, chemical analysis reveals that the concentration of NO2(g) is 0.010 M.(a) Calculate the number of moles of NO2(g).(b) Calculate the number of moles of N2O4(g) formed and its
A 100-L reaction container is charged with 0.50 mol NOBr, which decomposes at 120 °C.The equilibrium concentration of bromine is 2.0 × 10-3 M.(a) Calculate the concentrations of all species.(b) Calculate Kc. 1 NOBr(g) NO(g) + - Br(g) 2
A 2.00-L container at 463 K contains 0.500 mol phosgene. The equilibrium constant, Kc, is 4.93 × 10-3 forCalculate the concentrations of all species after the system reaches equilibrium. COC1(g) = CO(g) + Cl(g)
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 forCalculate the concentrations of all species after equilibrium has been reached. PC1; (g) PC13(g) + Cl(g)
Exactly 0.400 mol each of carbon monoxide and chlorine are sealed in a 2.00-L container at 919 °C. Kc is 7.52 forCalculate the concentrations of all species after equilibrium has been reached. CO(g) + Cl(g) COC1(g)
Consider a system that initially contains 0.100 mol each of phosphorus trichloride and chlorine sealed in a 10.0-L container. The temperature is increased to 291 °C where the equilibrium constant, Kc, is 8.18 forCalculate the concentrations of all species after the system reaches equilibrium.
Calculate the concentrations of all species formed when 1.00 mol sulfur dioxide and 2.00 mol chlorine are sealed in a 100.0-L reactor. The temperature is increased to 400 K, where Kc is 89.3 forCalculate the equilibrium concentrations of all species. SO(g) + Cl(g) SOCl(g) 14
Consider 1.00 mol carbon monoxide and 2.00 mol chlorine sealed in a 3.00-L container at 476 °C. The equilibrium constant, Kc, is 2.5 forCalculate the equilibrium concentrations of all species. (3)1DO) = (3)IO + ())
Exactly 2.00 atm carbon monoxide and 3.00 atm hydrogen are placed in a reaction vessel. Kp is 5.6 forCalculate the equilibrium pressures of all species. CO(g)+H,(g)=CH,O(g)
When lead iodate, Pb(IO3)2, is added to water, a small amount dissolves. If measurements at 25 °C show that the Pb2+ concentration is 4.5 × 10-5 M, calculate the value of Ksp for Pb(IO3)2.StrategySolubility equilibria are solved by the same approach used for all equilibria. We will write the
The solubility of La(IO3)3 is 7.3 × 10-4 M at 25 °C. Calculate the solubility product constant.
Calculate the solubility product constant for silver sulfate, given that the experimentally measured solubility is 0.44 g/100 mL. (Many solubility tables, such as those published in the Handbook of Chemistry and Physics, express solubility in grams per 100 mL of water, not moles per
Calculate the solubilities of AgIO3 and La(IO3)3 from their solubility product constants.
Given the value of Ksp, calculate the solubility of barium iodate, Ba(IO3)2.StrategyWrite the chemical equation, iCe table, the expression for Ksp, and solve.
Which of the solutions will show a common ion effect when the precipitate is lead bromide?
Which systems illustrate the common ion effect?StrategyLook at the precipitate, identify the cation and anion, and look to see whether either is present in the solution. Precipitates A. Mercury(I) chloride B. Barium sulfate Solutions 1. Barium chloride 2. Lead nitrate 3. Lithium sulfate 4.
Write(a) The equilibrium constant expression needed to determine the solubility of AgCl (Ksp = 1.8 × 10-10) in 1.0 × 10-5 M KCl(b) The resulting polynomial.
Complete the iCe table, write the expression for the solubility product constant needed to calculate the solubility of silver iodide (Ksp = 8.5 × 10-17) in a 0.10 M sodium iodide solution, and write the polynomial form of the equilibrium constant expression.StrategyThe same five-step approach
Calculate the solubility of CaF2 in 0.025 M NaF.
What is the solubility of calcium hydroxide (Ksp = 5.0 × 10-6) in 0.080 M sodium hydroxide solution?StrategyWrite the chemical equation, the iCe table, and the algebraic expression; substitute; and solve.
A chemist mixes 200 mL of 0.010 M Pb(NO3)2 with 100 mL of 0.0050 M NaCl. Will lead(II) chloride precipitate?StrategyDetermine Q and compare it with Ksp to determine whether lead chloride will form. 200 mL of 0.010 M Pb(NO3)2 300 200 100 100 ml. of 0.0050 M NaCl 300 -200 -100 300 mL of solution
The equilibrium system of hydrogen, nitrogen, and ammonia can be written in several different ways:The equilibrium constant, Keq, for reaction 1 is 0.19 at 532 °C. Write the equilibrium constant expression and calculate Keq for reactions 2 and 3 at the same temperature.StrategyFirst, write the
Use the preceding data to calculate Keq at 532 °C for 2 (8)H + (8)N (3) HN (9)N : 1.
Consider the equilibriumStrategyCompute Δn from the chemical equation, then rearrange the relationship Kp = Kc(RT)Δn to solve for Kc. Be sure to use 0.08206 L atm/mol K for R and express the temperature in kelvins. PC15(g) PC13(g) + Cl(g) If the numerical value of Kp is 0.74 at 499 K, calculate
Kp for the formation of 2 mol ammonia from nitrogen and hydrogen is 2.8 × 10-9 at 298 K. Calculate Kc for N(g) + 3H(g) 2NH3(g)
A scientist mixes 0.24 mol NO2 with 0.080 mol N2O4 in a 2.0-L flask at 418 K. Does a reaction occur to form more NO2, more N2O4, or is the system at equilibrium?
A scientist mixes 0.50 mol NO2 with 0.30 mol N2O4 in a 2.0-L flask at 418 K. At this temperature, Kc is 0.32 for the reaction of 2 mol NO2 to form 1 mol N2O4. Does a reaction occur to form more NO2 or more N2O4, or is the system at equilibrium?StrategyWrite the chemical equation and the expression
In which direction does the reaction proceed when sulfur dioxide is added to an equilibrium mixture of oxygen, sulfur dioxide, and sulfur trioxide?StrategyLe Chatelier’s principle predicts that the reaction will change in the direction that minimizes the change. 2 (8)OS (8)0 + (8) OS 1
In which direction does the reaction proceed when oxygen is removed from an equilibrium mixture of oxygen, sulfur dioxide, and sulfur trioxide? SO(g) + O(g) SO3(g) 12/0(g) =
Some PCl5 is placed in a 10.0-L reaction cylinder. The temperature is increased to 500 K, and the following reaction reaches equilibrium.In which direction does the system react if the external pressure increases, causing the volume to decrease to 1.0 L whereas the temperature is kept constant at
Ammonia is formed by the reaction of nitrogen and hydrogen, all in the gas phase . After the system reaches equilibrium, the volume of the container is decreased. In which direction does the reaction proceed? (N + 3H2NH3).
How does an increase in temperature influence each of the following equilibria?StrategyThe reaction will shift in the direction that minimizes the change. Heat can be considered a product in an exothermic reaction and a reactant in an endothermic reaction. (a) H(g) + 12(g) 2HI(g) (b) N(g) + 3H(g)
ΔH is -108 kJ for the formation of phosgene at the normal reaction temperature in Bhopal.In which direction does the system react if temperature is increased? CO(g) + Cl(g) COCI(g)
Exactly 0.00200 mol hydrogen iodide is placed in a 5.00-L flask, and the temperature is increased to 600 K. Some of the HI decomposes, forming hydrogen and the violetcolored iodine gas:After the system reaches equilibrium, the concentration of iodine is determined by measuring the absorption of
A researcher places 0.0400 mol sulfuryl chloride in a 4.00-L reactor. The temperature is increased to 100 °C, and some of the sulfuryl chloride decomposes to sulfur dioxide and chlorine.At equilibrium, the concentration of chlorine is found to be 3.9 × 10-3 M. Calculate Kc for this reaction.
At very high temperatures, Kc is 0.200 forCalculate the equilibrium concentrations of all species if the reaction starts with 5.00 × 10-4 mol NO in a 10.0-L container. 12 N(g) + O(g) 2NO(g)
Calculate the equilibrium concentrations of hydrogen and iodine that result when 0.050 mol HI is sealed in a 2.00-L reaction vessel and heated to 700 °C. At this temperature, Kc is 2.2 × 10-2 forStrategyWrite the chemical equation, iCe table, and algebraic expression for Keq; then substitute
Kc is 0.12 at 1000 K for the dissociation of phosgene:Calculate the equilibrium concentrations of all species if 2.00 mol COCl2 is placed in a 5.00-L reactor at 1000 K. COC12(g) CO(g) + Cl(g)
Phosphorus trichloride and chlorine react to form phosphorus pentachloride. At 544 K, Kc is 1.60 forCalculate the concentration of chlorine when 1.00 L of 0.600 M PCl3 is added to 2.00 L of 0.150 M Cl2 and allowed to reach equilibrium at 544 K.StrategyWrite the chemical equation, iCe table,
Write the iCe table and the expression for the equilibrium constant needed to solve for the concentrations of the species when 0.010 M SO2, 0.050 M O2, and 0.0020 M SO3 react. At 1009 K, Kc is 2.0 for 2SO(g) + O(g) = 2SO3(g)
A researcher studies an industrial process by placing 0.030 mol sulfuryl chloride, a powerful chemical oxidizer, in a 100-L reactor together with 2.0 mol SO2 and 1.0 mol Cl2 at 173 °C. At this temperature, Kp is 3.0 forWrite the iCe table and derive a polynomial algebraic expression needed to
Write the expressions for Kp and Kc for C(s) + HO(g) CO(g) + H(g)
Write the expressions for both Kp and Kc for the following reactions:StrategyRemember that pure solids and liquids do not appear in the expression for the equilibrium constant. (a) NaOH(s) + CO(g) NaHCO3(s) (b) KOH(s) + SO3(g) KHSO4(s) (c) NH4Cl(s) HCl(g) + NH3(g)
Write the solubility product expression for iron(III) hydroxide.
Write the chemical equation and expression for the solubility product constant for each of the following compounds:StrategyWrite the chemical equation for the solid dissolving; then write the expression for Ksp. (a) Mg(OH)2 (b) Ca3(PO4)2
When mercury(II) iodide dissolves in water, the concentration of mercury(II) ions is found to be 2 × 10-10 M. Calculate the solubility product constant for HgI2. The chemical equation is Hgl(s) Hg2+ (aq) + 21 (aq)
Write the Lewis symbol for the following species.(a) A sodium atom(b) A fluorine atom(c) O2(d) Mg2
Use valence bond theory to predict the planar shape of ethylene, C2H4.
Give the bonded-atom lone-pair arrangement expected for a central atom that has(a) Two bonded atoms and one lone pair.(b) Three bonded atoms and two lone pairs.(c) Four bonded atoms and two lone pairs.(d) Five bonded atoms and one lone pair.
Give the bonded-atom lone-pair arrangement and the shape of the following species.(a) XeO2(b) I−3(c) NO−2 (d) PCl5(e) AlCl3
Write a Lewis structure for each of the following species. Indicate all of the bond angles as predicted by the VSEPR model. Deduce the skeleton structure from the way each formula is written. (a) SO (b) CIO3 (c) SCN-
Indicate which molecules are polar and which are nonpolar.(a) SeO2(b) N2O (N is the central atom)(c) SCl4
Identify the hybrid orbitals on the nitrogen atoms that form the σ bonds in the following species.(a) HNCl2(b) NO−3(c) N2H2
Write the molecular orbital electron configuration and determine the bond order and number of unpaired electrons for the following ions.(a) C+2(b) N−2(c) Be−2
From the heating curves, which of the two substances, A or B, has the greater enthalpy of fusion?
Use the data in Figure 13.1 to fi nd the instantaneous rate of disappearance of the reactant at 20 seconds.Figure 13.1 Concentration of reactant (M) 1.0 0.8 0.6 0.4 0.2 0.0 + 0.0 5.0 10.0 15.0 Time (s) 20.0 25.0 30.0
Use the data in Figure 13.1 to calculate the instantaneous rate of disappearance of the reactant at 10 seconds.StrategyThe instantaneous rate is the slope of the tangent, so place a ruler on the graph, draw the tangent, and calculate the slope. Although two people might not place the ruler in
When 0.030 mol HCl dissolves in 100.0 g benzene, the solution freezes at 4.04 °C. When 0.030 mol HCl dissolves in 100.0 g water, the solution freezes at -1.07 °C. Use the data in Table 12.4 to complete the following exercises.Table 12.4(a) From the freezing point, calculate the molality of HCl in
Consider the formation of ammonia from the elements:(a) If the ammonia concentration is increasing at a rate of 0.024 M/s, what is the rate of reaction?(b) What is the rate of disappearance of hydrogenStrategyUse the rate of change of ammonia and the stoichiometry of the chemical equation to
Define rate law, rate constant, and reaction order.
Under different conditions, the rate of disappearance of N2 was 0.14 M/s N2. What is the rate of reaction? What is the rate of disappearance of hydrogen?
What are the units for the zero-, first-, and second-order rate constants?
If experiments show that the reaction ofStrategyThe order is the exponent to which the concentration is raised in the rate law, so we can look at the rate law, note the exponent, and state the order. NO(g) + 2O2(g) NO(g) + O3(g) follows the rate law rate = k[NO][0], what is the order in each
If the rate law is rate = k[NO]1/2[O2]2, what is the order in each species?
The following table gives the results of a similar experiment for the reaction of t-butyl bromide, (CH3)3CBr, with hydroxide ion. Calculate the rate law and the rate constant. (CH3)3CBr + OH- (CH3)3COH + Br Experiment 1 23 3 Initial Concentration (M) [OH-] 0.010 0.020 0.010 (CH3)3CBr 0.050 0.080
When methyl bromide reacts with hydroxide ion in solution, methyl alcohol and bromide ion form.Determine the rate law and evaluate the rate constant from the experimental data.StrategyAn information flow diagram helps to illustrate the problem-solving strategy. First, calculate relative
What is the difference between the integrated and differential forms of the rate law?
Determine the rate law (order and rate constant) from the data on the next page, obtained in a research laboratory that studies fast reactions. Assume that the reaction isStrategyFirst, determine the rate law for the reaction using the strategy shown in the block diagram. Th e core of our strategy
Explain how to use the method of initial rates to determine the rate law for CH3Br + OH CH3OH + Br
Graph the data in the table to determine whether the reaction is zero order, first order, or neither.
Explain why half-lives are not normally used to describe reactions other than first order.
Derive an expression for the half-life of a reaction with a half-order rate law from the following integrated rate law: [R]/ = [R]/2 - 1/2 kt
What is the concentration of fenvalerate in the pond 1 year (3.15 × 107 s) after the spill?
The pesticide fenvalerate, C25H22ClO3N, is a member of a class of compounds called pyrethrins. Fenvalerate is one of four compounds approved by New York City to combat the mosquitoes that spread West Nile virus. These compounds were originally isolated from plants (including chrysanthemums) that
Derive an expression for the half-life of a reaction with the following third-order rate law: 1 2 [R]. 1 [R] = 2kt
Dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen. When the reaction takes place in carbon tetrachloride (CCl4), both nitrogen oxides are soluble, but the oxygen escapes as a gas.The rate of reaction (-Δ[N2O5]/Δt) can be measured by monitoring the volume of oxygen gas that is
In this experiment, how long does it take for the N2O5 to decrease from 0.015 to 0.010 g?
A piece of wood has 25% of the 14C originally present. How old is the wood?
The decomposition of HI at 117 °C is measured in the laboratory.What are the rate law and the rate constant? 2HI(g) H(g) + 1(g)
Nitrogen dioxide decomposes to nitrogen monoxide and oxygen in a second-order reaction.The decrease in concentration of NO2 is shown as a function of time in the accompanying figure. Use the data to calculate the rate constant for the reaction.StrategyBecause we are told that the reaction is second
The age of Ötzi, the Ice Man, discussed in the chapter introduction, was determined by carbon-14 (14C) dating. 14C is a radioactive isotope with a half-life of 5730 years. A sample of carbon-containing material was found to have 52.7% of its original amount of 14C. Use this information to
List the factors that affect the rate of reaction.
Determine the rate law and rate constant for the decomposition of the organic compound 1,3-pentadiene.1,3-pentadiene → productsThe concentration of 1,3-pentadiene was measured as a function of time. The data are as follows:StrategyA logic flow diagram shows the strategy. We will prepare up to
Determine the rate law and rate constant for the reaction R products [R] (M) 0.43 0.25 0.17 0.13 0.11 Time (s) 0.0 2.0 4.0 6.0 8.0
The number of collisions per second that have energies exceeding the activation energy can be determined. Explain how this determination is or is not useful in predicting the rate of a chemical reaction.
Sketch the energy-level diagram for an endothermic reaction with low activation energy and for an exothermic reaction with high activation energy.
Consider the decomposition of nitrogen dioxide.At 650 K , the rate constant is 1.66 L/mol · s ; at 700 K , it is 7.39 L/mol · s . Use these rate constants to determine the activation energy.StrategyEquation 13.11 relates two rate constants and two temperatures. Let subscript 1 in Equation 13.11
Calculate the activation energy (in kJ/mol) for a reaction that has k = 1.0 × 108 s-1 at 250 K and k = 3.8 × 108 s-1 at 350 K.
A reaction rate doubles when an investigator increases the temperature by 10 °C, from 298 to 308 K . What is the activation energy?StrategyStart with Equation 13.11:To solve this problem, we need to recognize that the ratio k1/k2 is 1:2 because we are told that the rate doubles. Because we are
Explain the effect of doubling the concentration of one reactant on the collision frequency.
The rate of a reaction doubles when the temperature changes by 15 °C, from 298 to 313 K. Calculate the activation energy for the reaction.
Evaluate the proposed mechanism (all substances are gases) to determine the overall stoichiometry. Identify intermediates. NO + NO NO3 + NO NO3 + CO NO + CO Step 1 Step 2
The gas-phase reaction of nitrogen dioxide with fluorine proceeds to form nitrosyl fluoride, NO2F.Determine whether the following mechanism provides the correct overall stoichiometry, and identify intermediates, if any.StrategySum the proposed elementary steps to determine whether these steps
Define activation energy, and explain how it influences the rate of reaction.
Write the rate law and expected molecularity for the overall reaction: CH4 + 202 CO + 2HO
Explain why a collision must exceed a minimum energy for a product to form.
Write the expected rate law and molecularity for each of the following elementary reactions in the gas phase.StrategyThe rate law for an elementary reaction is derived directly from its stoichiometry. The molecularity is the sum of the exponents of the concentrations in the elementary step. (a) HCl

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