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introductory chemistry atoms first

Questions and Answers of Introductory Chemistry Atoms First

What does a catalyst do to the time it takes for a reaction to reach equilibrium? Explain how it does this.
Write the equilibrium constant expression for (a) 2 FeCl3(s) + 3 H₂O(g) (b) Fe₂O3(s) + 3 CO(g) → (c) PbSO(s) Pb²+ (aq) + SO3(aq) Fe₂O3(s) + 6 HCI(g) 2 Fe(1) + 3 CO₂(g) (d) CO₂(g) +
As noted in the chapter, the value of Keq for the reaction N2(g) + O2(g) ⇄ 2 NO(g) is 0.0017 at 2027 °C and 2.3 × 10–9 at 25 °C.(a) Judging from the values of Keq, does this reaction shift to
Write the equilibrium constant expression for (a) SnO₂(s) + 2 H₂(g) Sn(s) + 2 H₂O(1) (b) H3PO4(aq) + 3 H₂O(1) ⇒ PO (aq) 2+ (c) Pb²+ (aq) + 21 (aq) +3HgO*(aq) Pbl₂(s) (d) Ca²+ (aq) + 3
What is a heterogeneous chemical reaction? Where does a heterogeneous reaction occur?
What allows us to incorporate the concentrations of pure solids and liquids into Keq instead of writing these concentrations explicitly in the equilibrium constant expression?
Consider the reactionrun in an explosion-proof sealed vessel.(a) Running the reaction in a sealed vessel allows equilibrium to be established. Explain why.(b) Express the concentration of H2(g) in
Consider a saturated aqueous solution of AgCl, a salt that is only sparingly soluble in water. What happens to this solution if a saturated solution of NaCl (a water-soluble salt) is added to it?
What is the most soluble 1:2 salt in Table 14.1? Explain how you know. Table 14.1 Solubility Products of Some Ionic Compounds at 25 °C Molecular formula Pbl₂ Compound Aluminum hydroxide Barium
What is “dynamic” about the equilibrium that is established when a sparingly soluble salt is added to water?
At 25 °C, the solubility of Al(OH)3 in water is 2.86 × 10–9 M. What are the equilibrium concentrations of the cation and the anion in a saturated solution?
At 25°C, the solubility of Ca3(PO4)2 in water is 2.60 × 10–6 M. What are the equilibrium concentrations of the cation and the anion in a saturated solution?
At 25 °C, the solubility in water of the moderately soluble salt silver acetate, AgC2H3O2, is 10.6 g/L.(a) Write the chemical equation for the dissolving of silver acetate in water.(b) Write the Ksp
At 25 °C, the solubility of calcium oxalate, CaC2O4, in water is 6.1 mg/L.(a) What are the equilibrium molar concentrations of Ca2+ (aq) and C2O42–(aq)?(b) Calculate Ksp for calcium oxalate.
At 25 °C, the solubility of iron(III) hydroxide in water is 4.49 × 10–10 M.(a) What is the solubility in grams per liter?(b) What is the molar equilibrium concentration of each ion?(c) How many
At 25°C, what is the solubility of lead(II) carbonate in water:(a) In moles per liter?(b) In grams per liter?(c) What is the molar equilibrium concentration of each ion?(d) How many grams of
Tin(II) sulfide, SnS, is dissolved in an aqueous solution in which the Sn2+ concentration is fixed at 2.00 × 10–1 M. What is the sulfide concentration?
In the Haber process, nitrogen gas reacts with hydrogen gas to form gaseous ammonia (see Problem 14.76).(a) Write the equilibrium expression for the reaction.(b) The equilibrium constant at a certain
Phosphorus pentachloride gas decomposes to PCl3(g) and Cl2(g). At equilibrium, the concentrations of the decomposition products are 5.50 × 10–3 M for PCl3(g) and 0.125 M for Cl2(g). What is the
Suppose the reaction A2 + B2 ⇆ 2 AB proceeds via a one-step mechanism involving a collision between one A2 molecule and one B2 molecule. Suppose also that this reaction is reversible, and that the
Suppose the reaction in Problem 14.105 goes to completion. What must be true about Ea for the forward reaction relative to Ea for the reverse reaction?Data from Problem 14.105Suppose the reaction A2
For the reactionKeq = 0.500. What is the equilibrium molar concentration of NO2(g) if [N2O4] = 0.248 M? 2 NO₂(8) N₂O4(8)
When the reaction N2(g) + O2(g) ⇆ 2NO(g) is run at 2000 °C, appreciable amounts of reactants and product are present at equilibrium.(a) A sealed 2.00-L container at 2000 °C is filled with 1.00
Write the equilibrium constant expression for: (a) SiC14 (1) + 2 H₂O(g) (b) H₂(g) + CO₂(g) — CO(g) + H₂O(1) (c) MnO₂(s) + 4H* (aq) + 2 Cl(aq) SiO₂ (s) + 4 HCl(g) Mn²+ (aq) + Cl₂(g) +
For an endothermic reaction, will the equilibrium constant increase, decrease, or stay the same as the temperature of the reaction mixture increases? Explain your answer.
After the reaction N2(g) + 3H2(g) ⇆ 2 NH3(g) is run, an equilibrium mixture at 300 °C is 0.25 M in N2(g), 0.15 M in H2(g), and 0.090 M in NH3(g).(a) What is the value of Keq?(b) Which way does the
Hydrochloric acid is added to an aqueous solution of silver nitrate.(a) What precipitate forms?(b) The equilibrium concentration of Cl–(aq) is 2.0 × 10–3 M. What is the equilibrium concentration
The solubility of silver acetate in water at 20 °C is 10.5 g/L of solution. Calculate Ksp for silver acetate.
How many moles of BaSO4 will dissolve in 200.0 mL of water at 25°C?
The solubility of PbI2 in water at 25 °C is 1.52 × 10–3 M. How many grams of PbI2 will dissolve in 2.50 × 106 gallons of water at 25 °C?
For the reactionat 25 °C, Keq = 0.150. What is the equilibrium concentration of NO2(g) if [N2O5] = 0.300 M and [O2] = 1.20 M? 4 NO₂(g) + O₂(8) 2N₂O5(8)
(a) How would you prepare a saturated aqueous solution of copper(I) iodide at 25 °C?(b) What is the mass in milligrams of CuI in 400.0 mL of the saturated solution?(c) Suppose you add some CuI* to
Which of the following reactions is described by the equilibrium constant expression [A]²x [B]³ [C]³X [D]² Keq (a) A2+B3 (b) 2A + 3B 3C + 2D (c) 3C + 2D2A + 3B (d) A²+ B³ C³ + D² (e) 2C +
In which direction does the reactionshift when:(a) (CO2) is increased?(b) The volume of the reaction vessel is decreased?(c) Ca2+ (aq) is added?(d) CaCO3(s) is removed? CaCO3(s) + H₂O(1) +
Would the solubility of PbI(s) be greater in water or in an aqueous solution of NaI? Explain your answer.
Keq = 3.9 × 10–11 for the dissolution of calcium fluoride in water:(a) What is another name for Keq for this reaction?(b) If the equilibrium calcium ion concentration in a saturated aqueous
A reaction at equilibrium is disturbed as shown and then returns to equilibrium. The temperature remains constant.(a) How do the values of Keq compare for the initial and new equilibria?(b) Something
Consider the following reaction energy profile:(a) At a given temperature, which is faster, the forward reaction or the reverse reaction? Explain how you knew.(b) Based on your answer to (a), is kf
Consider the two curves, one showing supply of tapes, the other showing demand for tapes. At what price per quantity is equilibrium established? Price (dollars per tape) 6 LO 5 4 3 2 1 0 Supply of
The following plot traces the concentrations over time for the reactant and product in the equilibrium reaction N2O4(g) ⇆ 2NO2(g). At approximately what time into the reaction has equilibrium
A sealed 1-L flask is filled with 1 mole of H2(g) and 1 mole of I2(g). The reversible reaction H2(g) + I2(g) → 2HI(g) ensues. A plot showing what happens to the HI concentration as a percent of the
Some liquid water is placed in a room-temperature container and sealed. After some time, the level of the liquid drops by a small amount. After that, the water level remains constant.What does this
Consider the reversible reaction shown below:Instead of using molar concentrations, you can use gas pressures to calculate an equilibrium constant, in which case it is often labeled Kp instead of
Consider the gas-phase reaction:Suppose it is at equilibrium inside of a closed vessel. Next, the volume of the closed vessel is suddenly decreased, increasing the overall pressure inside the flask.
The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43 × 10–3 g/L at 25 °C.(a) Write a balanced equation for the solubility equilibrium.(b) Write the expression for Ksp and calculate its
In theory, all reactions are reversible, but in practice, some are not. Explain why.
Shown below is a concentration versus time plot for the reaction A ⇆ B. Using the data on the graph, determine the equilibrium constant for the reaction. Concentration
Indicate with an arrow the direction of the equilibrium shift and predict what will happen to the amount of Fe2O3 (increases, decreases, unchanged, need more information) when the following stresses
How does decreasing the temperature affect the value of Keq for an exothermic reaction?(a) Increases Keq(b) Decreases Keq(c) Does not change Keq
The Keq for the equilibrium below is 0.112 at 700.0 °C.What is the value of Keq at this same temperature for the following reaction? SO₂(8) + 1/2O₂(g) → SO3(8)
Consider the reaction between NH3 andDiscuss what will happen when these two molecules meet, and write a chemical reaction showing the products. Then apply an appropriate acid–base theory so you
A substance is an electrolyte if:(a) It conducts electricity.(b) It can produce electricity.(c) An aqueous solution of it conducts electricity.(d) It is a neutral substance.
Of the three solutions shown here, (a) Which is a weak electrolyte, which is a strong electrolyte, and which is a nonelectrolyte? How can you tell?(b) Which of these compounds is/are molecular?
(a) Is the compound H2SO4 molecular or ionic?(b) How did you decide on your answer to part (a)?(c) Based on your answer to part (a), would you call H2SO4 an electrolyte or a nonelectrolyte?(d) An
Sodium bicarbonate has the formula NaHCO3, and in solution, it gives aqueous Na+ ions and aqueous HCO3– (bicarbonate) ions.(a) Is the HCO3– ion the conjugate base of carbonic acid (H2CO3)?
To be an electrolyte, a compound:(a) Must be insoluble in water.(b) Must dissolve in water and produce electricity.(c) Must dissolve in water and yield electrons.(d) Must dissolve in water and
Sulfuric acid, H2SO4, is a diprotic acid. Write a balanced equation for sulfuric acid dissolving in water, showing the maximum number of H3O+ ions it can produce.
Indicate whether each compound is an electrolyte or a nonelectrolyte in water:(a) Al(NO3)3(b) (CH3)2O(c) (NH4)2SO4(d) CH3OH(e) CuSO4(f) KBr(g) HBr
(a) What species are present in each beaker?(b) Ionic compounds are often called salts. What are the chemical formula and name of the salt that gives rise to the salt solution in beaker 3? 1. Aqueous
The following statement is true regarding dissociation into ions upon dissolving in water.(a) Only soluble ionic substances also dissociate into ions.(b) Only soluble molecular substances also
(a) Draw a beaker containing water and show what ions, if any, are present when ammonium bromide, NH4Br, dissolves.(b) Does the NH4Br dissociate? What does the fact that it does or does not
Which one of these three molecules can act as a base according to the Brønsted–Lowry definition? Explain your answer. (a) H H CIH H CH4 H (b) H H PH3 H (c) H H B BH3 H
For a substance to be a weak electrolyte, the following must be true:(a) The substance must be nearly insoluble in water.(b) The equilibrium for dissociation must lie far to the right.(c) “The
True or false? If a compound is a molecular substance and an acid in water, it must also be an electrolyte.
Go back and examine Equation 15.4, where a hydroxide ion reacts with a hydronium ion, and then answer these questions:(a) Use the Brønsted–Lowry definition of a base to explain why it is proper to
To be an acid, a substance must:(a) Be an electrolyte.(b) Dissociate in water to produce hydronium (H3O+) ions.(c) Be able to neutralize bases.(d) All of the above statements are correct.
Write a balanced dissociation equation for carbonic acid in water that shows the maximum number of H3O+ ions the acid can yield.
The reactionis run at one temperature in flask (a) and at a different temperature in flask (b). Which flask is at the lower temperature, and which is at the higher temperature? Explain your answer.
An acid is considered to be weak if:(a) It cannot neutralize a base.(b) It does not burn the skin.(c) Its equilibrium for dissociation lies far to the left.(d) It cannot produce hydronium (H3O+) ions.
Your answer to Practice Problem 15.5 shows the dissociation yielding 2 moles of protons per mole of acid, but this reaction actually produces fewer protons. Write the two balanced equilibrium
For each solution, determine [OH–] and decide whether the solution is acidic, basic, or neutral. Arrange your results in tabular form. Solution 1 2 234 4 5 67 7 8 9 10 1122 13. 14 15 [H3O+] 10⁰
NH3 (ammonia) is considered a weak base because:(a) It contains no hydroxide (OH–) ions like NaOH does.(b) It accepts a proton from water to produce hydroxide ions in a left-lying equilibrium.(c)
Determine the unknown concentration in each solution, and then decide whether the solution is acidic or basic. Why did you decide as you did? (a) [H₂O+] = 2 M [OH-] = ? (b) [H₂O+] = ? [OH-] = 4 M
What salt forms when sulfuric acid completely neutralizes sodium hydroxide? Give both name and formula for the salt.
A sample of pure water:(a) Contains only water molecules and nothing else.(b) Also has hydronium (H3O+) ions in it at a concentration of 10–14 M.(c) Also has hydroxide (OH–) ions in it at a
How many moles of NaOH would it take to neutralize 1 mole of hydrochloric acid? How many moles of NaOH would it take to neutralize 1 mole of sulfuric acid? Why aren’t the answers to these two
An aqueous solution that has an H3O+ concentration of 10–8 M is (a) Acidic.(b) Basic.(c) Neutral.(d) There is so little H3O+ that the question cannot be answered.
What is the conjugate base of citric acid, C5H7O6OH?
A basic solution has a pH of 9.8. What is its molar H3O+ concentration?
What is the H3O+ concentration in a solution that is 100 times less acidic than one having a pH of 2.56?
What is the OH– concentration in a solution having a pH of 5.55?
(a) Show how HCO3– can act as a weak acid.(b) Show how HCO3– can act as a weak base.(c) Since HCO3– can act as either an acid or a base, can it be its own conjugate?
If HCO3– is considered a weak acid, what is its conjugate base?
If HCO3– is considered a weak base, what is its conjugate acid?
Ammonium ion, NH4+, is a weak acid. Write the equation for its reaction with water.
Ammonia, NH3, is a weak base. Write the equation for its reaction with water.
What do you call an aqueous solution that contains a large amount of dissolved NH4Cl and NH3? Explain.
Write a reaction to show how the solution in Practice Problem 15.39 resists pH change when OH– ions are added.Data from Problem 15.39What do you call an aqueous solution that contains a large
Write a reaction to show how the solution in Practice Problem 15.39 resists pH change when H3O+ ions are added.Data from Problem 15.39What do you call an aqueous solution that contains a large amount
List the three criteria early chemists used to classify a compound as an acid.
List the three criteria early chemists used to classify a compound as a base.
To be an indicator, what must a compound do? Give an example of one and explain how it behaves.
What is an electrolyte? What is a nonelectrolyte? Give some examples of each.
Describe an experimental setup to determine whether a compound is an electrolyte or a nonelectrolyte. What would you look for?
Ethanol, C2H5OH, dissolves in water. So does magnesium chloride, MgCl2. Yet there is a fundamental difference in the way these two substances dissolve. What is this fundamental difference?
What is the difference between just dissolving versus dissolving and dissociating? Give an example of each.
If an ionic compound is water-soluble, it is an electrolyte. Explain why.
True or false? Because the solid phase of a molecular compound does not consist of ions, the compound cannot dissociate into ions when it dissolves in water. Back up your answer with an explanation
Electricity can be defined as charged particles in motion. Using this definition, explain how an aqueous solution of an electrolyte conducts electricity.
The molecular compound HCl is an electrolyte.(a) What do we mean when we say that HCl is a molecular compound?(b) Is it incorrect to call HCl an ionic compound?(c) What must a molecular compound like

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