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introductory chemistry concepts

Questions and Answers of Introductory Chemistry Concepts

Which of the following classes of compounds has a carbonyl group?(a) Aldehyde(b) Amide(c) Ester(d) Ketone(e) All of the above.
Two antacid tablets are taken orally—one contains magnesium hydroxide and the other aluminum hydroxide. If each tablet contains 500 mg of antacid, what is the total volume of 0.100 M HCl
Sodium bicarbonate and aluminum hydroxide are found in antacid tablets. Which antacid tablet neutralizes the most 0.100 M HCl stomach acid: a tablet containing 1.00 g NaHCO3 or a tablet with 1.00 g
What is the mass of a 1.00-inch cube of magnesium (d = 1.74 g/cm3)?(a) 0.575 g(b) 1.74 g(c) 9.43 g(d) 16.4 g(e) 28.5 g.
Estimate an approximate answer for each of the following calculations. Verify your ballpark answer using a calculator. (a)(b) 39.50 mL AlCl3 X 278.1 g PbCl2 1 mol PbCl₂ 0.115 mol AlCl3 1000 mL
How many water molecules are in a 1.00-mm3 cube of ice (d = 0.917 g/cm3 )?(a) 9.17 x 10-4 molecules(b) 3.06 x 1019 molecules(c) 3.06 x 1022 molecules(d) 5.09 x 1018 molecules(e) 5.09 x 1020
If a pencil manufacturer produces 288,125 pencils, how many gross of pencils can be sold? (A gross is 144 pencils.)
If a paper manufacturer produces 4,125,365 sheets of paper, how many reams of paper can be sold? (A ream is 500 sheets.)
Given that 45.0 mL of nitrogen gas react with 65.0 mL of oxygen gas according to the unbalanced equation: N2(g) + O2(g) → NO2(g) (a) What is the limiting reactant?(b) Assuming constant
Given that 25.0 L of sulfur dioxide reacts with 25.0 L of oxygen gas according to the unbalanced equation: SO2(g) + O2(g) → V2O5/650 °C SO3(g) (a) What is the limiting reactant?(b) Assuming
Given that 1.00 g of aluminum hydroxide react with 25.0 mL of 0.500 M sulfuric acid according to the unbalanced equation: Al(OH)3(s) + H2SO4(l) → Al2(SO4)3(aq) + H2O(l)(a) What is the limiting
Given that 36.5 mL of 0.266 M calcium acetate react with 25.0 mL of 0.385 M sodium carbonate according to the unbalanced equation: Ca(C2H3O2)2(aq) + Na2CO3(aq) → CaCO3(s) + NaC2H3O2(aq)(a) What
Seawater contains approximately 1.22 x 1010 atoms of gold per milliliter. How many kilograms of seawater must be evaporated to obtain 12.0 g of gold? (Assume the density of seawater is 1.05 g/mL.)
The volume of the oceans is 1.4 x 1021 liters. Calculate the mass of chlorine in all seawater given the mass percent concentration of chloride ion is 1.90%. (Assume the density of seawater is 1.05
What is the molar sodium ion concentration resulting from mixing of 50.0 mL of 0.100 M sodium chloride and 50.0 mL of 0.200 M sodium sulfate?
A sample of sodium carbonate is treated with 50.0 mL of 0.345 M HCl. The excess hydrochloric acid is titrated with 15.9 mL of 0.155 M NaOH. Calculate the mass of the sodium carbonate sample.
What is the molar chloride ion concentration resulting from mixing of 50.0 mL of 0.100 M sodium chloride and 25.0 mL of 0.100 M potassium chloride?
The chloride in an aqueous sample of BaCl2 is precipitated with 50.0 mL of 0.100 M AgNO3. The excess silver nitrate is titrated with 17.0 mL of 0.125 M K2CrO4. Calculate the mass of the barium
The president of a college reports to a board of trustees, and three vice-presidents report to the college president. The chief financial officer reports directly to the board of trustees. Draw a
A computer application program can transfer information to a word processing document, a data base, and a spreadsheet. Draw a concept map for the computer application.
According to collision theory, which of the following factors influences the rate of a chemical reaction?(a) Frequency of molecular collisions(b) Energy of molecular collisions(c) Orientation of
State three experimental variables that can be changed to increase the rate of a chemical reaction.
Which of the following factors influences the rate of a chemical reaction?(a) Concentration(b) Temperature(c) Catalyst(d) All of the above(e) None of the above.
Which of the following theoretical factors decreases the rate of a reaction?(a) Decrease collision frequency(b) Decrease collision energy(c) Ineffective collision orientation.
Ultraviolet light from the Sun converts oxygen molecules in the upper atmosphere to ozone molecules. Draw the reaction profile for the reaction: 30₂(g) + heat UV 2 03(8)
Nitrosyl bromide, NOBr, decomposes to give nitric oxide and bromine gas. Draw the reaction profile for the reaction: 2 NOBr(g) ⇌ 2 NO(g) + Br2(g) + heat
If the heat of reaction is exothermic, which of the following is true?(a) The energy of the reactants is greater than the products.(b) The energy of the reactants is less than the products.(c) The
Which of the following theoretical factors increases the rate of a reaction?(a) Increase collision frequency(b) Increase collision energy(c) Effective collision orientation.
Write the equilibrium constant expression for the following reversible reaction. A + 2 B ⇌ 3 C + D
Write the equilibrium constant expression for the following reversible reaction. 2 A + 3 B ⇌ C + 4 D
Which of the following is true after a reaction reaches equilibrium?(a) The amount of reactants and products are equal.(b) The amount of reactants and products are constant.(c) The amount of
Draw a diagram showing an effective collision orientation between a hydrogen molecule and a bromine molecule.
Write the equilibrium constant expression for each of the following reversible reactions:(a) 2 NO(g) + 2 H2(g) ⇌ N2(g) + 2 H2O(g) (b) NH4NO3(s) ⇌ N2O(g) + 2 H2O(g)
Write the equilibrium constant expression for each of the following reversible reactions:(a) 4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6 H2O(g) (b) CaCO3(s) ⇌ CaO(s) + CO2(g)
Dinitrogen tetraoxide decomposes to produce nitrogen dioxide. Calculate the equilibrium constant for the reaction given the equilibrium concentrations at 100 °C: [N2O4] = 0.800 and [NO2] =
Draw a diagram showing an ineffective collision orientation between a hydrogen molecule and a bromine molecule.
We first write the equilibrium expression for the reaction. Second, we substitute the concentration values into the expression. The large Keq for this reaction indicates that the equilibrium
In the upper atmosphere, nitric oxide and nitrogen dioxide participate in the following equilibrium: 2 NO(g) + O2(g) ⇌ 2 NO2(g) Given the equilibrium concentrations for each gas at 25°C, what is
Which of the changes listed has no effect on the equilibrium for the following reversible reaction?CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + heat(a) Increase volume(b) Decrease volume(c) Add a
State the effect on the rate of reaction for each of the following.(a) Decrease the concentration of a reactant(b) Decrease the temperature of the reaction(c) Add an acid catalyst.
Charcoal reacts with steam according to the equation. C(s) + H2O(g) + heat ⇌ CO(g) + H2(g) Predict the direction of equilibrium shift for each of the following stresses:(a) Increase
Methane, CH4, reacts with limited oxygen according to the equation. 2 CH4(g) + O2(g) ⇌ 2 CO(g) + 4 H2(g) + heat Predict the direction of equilibrium shift for each of the following
If the hydrogen ion concentration of a 0.100 M HC3H5O3 solution is 0.0038 M, what is the ionization constant for lactic acid?(a) Ki = 1.4 x 10–3(b) Ki = 1.4 x 10–4(c) Ki = 1.4 x 10–5(d) Ki
State the effect on the rate of reaction for each of the following.(a) Increase the concentration of a reactant(b) Increase the temperature of the reaction(c) Add a metal catalyst.
Write the equilibrium constant expression for the following weak acid: HNO2(aq) ⇌ H+(aq) + NO2–(aq)
Write the equilibrium constant expression for the following weak acid: H2CO3(aq) ⇌ H+(aq) + HCO3–(aq)
Which of the changes listed has no effect on the equilibrium for the following reversible reaction in an aqueous solution? HC2H3O2(aq) ⇄ H+(aq) + C2H3O2–(aq)(a) Increase [HC2H3O2](b) Increase
The Contact Process uses a metal catalyst to produce sulfur trioxide gas for the manufacture of sulfuric acid. Does the catalyst increase the amount of sulfur trioxide gas? Explain.
Hydrofluoric acid, HF, ionizes according to the equation: HF(aq) ⇌ H+(aq) + F–(aq) Predict the direction of equilibrium shift for each of the following stresses:(a) Increase [HF](b) Increase
Hydrocyanic acid, HCN, ionizes according to the equation HCN(aq) ⇌ H+(aq) + CN–(aq) Predict the direction of equilibrium shift for each of the following stresses:(a) Increase
The Haber Process uses a metal oxide catalyst to produce ammonia gas. Does the catalyst increase the amount of ammonia gas? Explain.
What is the Ksp for silver carbonate, Ag2CO3, if the silver ion concentration in a saturated solution is 0.00026 M? (a) Ksp = 3.4 x 10–8(b) Ksp = 6.8 x 10–8(c) Ksp = 3.6 x 10–11(d) Ksp =
Write the solubility product expression for slightly soluble calcium phosphate in an aqueous solution. Ca3(PO4)2(s) ⇌ 3 Ca2+ (aq) + 2 PO4 3– (aq)
Write the solubility product expression for slightly soluble aluminum carbonate in an aqueous solution. Al2(CO3)3(s) ⇌ 2 Al3+ (aq) + 3 CO3 2– (aq)
Phosphorus pentachloride is used in the electronics industry to manufacture computer chips. Draw the energy profile for the following reaction. PCl5(g) + heat ⇄ PCl3(g) + Cl2(g)
Which of the changes listed below has no effect on the equilibrium for the following reversible reaction? Mg(OH)2(s) N Mg2+ (aq) + 2 OH–(aq)(a) Increase [Mg2+](b) Increase pH(c) Add sulfuric
A saturated solution of silver chloride dissociates according to the following equation: AgCl(s) ⇌ Ag+(aq) + Cl–(aq) Predict the direction of equilibrium shift for each of the following
State the substances undergoing oxidation and reduction in the following ionic redox reactions.(a) Al(s) + Cr3+(aq) → Al3+(aq) + Cr(s)(b) F2(g) + 2 Cl–(aq) → 2 F–(aq) + Cl2(g).
State the substances undergoing oxidation and reduction in the following ionic redox reactions.(a) Fe3+(aq) + SO3 2–(aq) → Fe2+(aq) + SO4 2–(aq)(b) Cl2(g) + 2 I–(aq) → 2 Cl–(aq) +
Indicate the oxidizing and reducing agents in the following redox reactions.(a) CuO(s) + H2(g) → Cu(s) + H2O(l)(b) PbO(s) + CO(g) → Pb(s) + CO2(g).
Indicate the oxidizing and reducing agents in the following redox reactions.(a) Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g) (b) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g).
Does the electron loss by oxidation always equal the electron gain by reduction in a balanced redox equation?
Does the total ionic charge on the reactants always equal the total ionic charge on the products in a balanced redox equation?
Write a balanced equation for each of the following redox reactions using the oxidation number method.(a) Br2(l) + NaI(aq) → NaBr(aq) + I2(s)(b) PbS(s) + O2(g) → PbO(aq) + SO2(g).
Write a balanced equation for each of the following redox reactions using the oxidation number method.(a) Cl2(g) + KI(aq) → I2(s) + KCl(aq)(b) Fe2O3(s) + CO(g) → Fe(s) + CO2(g).
Write a balanced equation for each of the following redox reactions using the oxidation number method.(a) MnO4–(aq) + I–(aq) + H+(aq) → Mn2+(aq) + I2(s) + H2O(l)(b) Cu(s) + H+(aq) + SO4
Write a balanced equation for each of the following redox reactions using the oxidation number method.(a) Fe2+(aq) + H2O2(aq) + H+(aq) → Fe3+(aq) + H2O(l)(b) Cr2O7 2–(aq) + Br–(aq) + H+(aq)
Write a balanced half-reaction for each of the following in an acidic solution.(a) H2O2(aq) → H2O(l)(b) AsO3 3–(aq) → AsO3–(aq).
Write a balanced equation for each of the following redox reactions in an acidic solution using the half-reaction method. (a) Zn(s) + NO3- (aq) (b) Mn²+ (aq) + BiO3(aq) Zn²+ (aq) + NO(g) MnO4
Write a balanced half-reaction for each of the following in a basic solution.(a) Ni(OH)2(s) → NiO2(s)(b) NO2–(aq) → N2O(g).
Write a balanced equation for each of the following redox reactions in a basic solution using the half-reaction method. (a) MnO4 (aq) + S²(aq) (b) Cu(s) + CIO (aq) MnO₂(s) + S(s) Cu²+ (aq) + Cl
Chlorine can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in an acidic solution. Cl2(aq) → Cl–(aq) + HOCl(aq)
Refer to Figure 17.4 and indicate which substance in each of the following pairs has the greater tendency to be oxidized.(a) Li(s) or K(s)(b) Al(s) or Mg(s)(c) Fe2+(aq) or I–(aq)(d) Br–(aq)
Chlorine can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in a basic solution. Cl2(aq) → ClO2–(aq) + Cl–(aq)
Refer to Figure 17.4 and indicate which substance in each of the following pairs has the greater tendency to be reduced.(a) Pb2+(aq) or Zn2+(aq)(b) Fe3+(aq) or Al3+(aq)(c) Ag+(aq) or
Refer to Figure 17.4 and indicate which substance in each of the following pairs is the stronger reducing agent.(a) Cu(s) or Cr(s)(b) H2(g) or Cu(s)(c) Cu(s) or I–(aq)(d) Cl–(aq) or
Refer to Figure 17.4 and indicate which substance in each of the following pairs is the stronger oxidizing agent.(a) F2(g) or Cl2(g)(b) Ag+(aq) or Br2(l)(c) Cu2+(aq) or H+(aq)(d) Mg2+(aq) or
Refer to Figure 17.4 and state whether each of the following reactions is spontaneous or nonspontaneous.(a) Br2(l) + LiF(aq) → F2(s) + LiBr(aq)(b) Al(NO3)3(aq) + Mn(s) → Mn(NO3)2(aq) +
Refer to Figure 17.4 and state whether each of the following reactions is spontaneous or nonspontaneous.(a) Cr(s) + HCl(aq) → CrCl3(aq) + H2(g) (b) FeCl3(aq) + NaI(aq) → FeCl2(aq) + NaCl(aq) +
Refer to Figure 17.4 and state whether each of the following ionic redox reactions is spontaneous or nonspontaneous.(a) Mg(s) + Sn2+(aq) → Mg2+(aq) + Sn(s)(b) H+(aq) + Ni(s) → H2(g) +
Refer to Figure 17.4 and state whether each of the following ionic redox reactions is spontaneous or nonspontaneous.(a) H+(aq) + I–(aq) → H2(g) + I2(s)(b) Fe3+(aq) + I–(aq) → Fe2+(aq) +
Sketch the following voltaic cell showing the two compartments, the anode and cathode, the wire connecting the two electrodes, and a salt bridge. Mn(s) + Cd(NO3)2(aq) → Cd(s) + Mn(NO3)2(aq)
Sketch the following voltaic cell showing the two compartments, the anode and cathode, the wire connecting the two electrodes, and a salt bridge. Ni(s) + 2 AgNO3(aq) → 2 Ag(s) + Ni(NO3)2(aq)
Diagram the direction of electron flow and the movement of nitrate ions in the salt bridge that connects the two half cells in Exercise 37.Exercise 37Sketch the following voltaic cell showing the two
Diagram the direction of electron flow and the movement of nitrate ions in the salt bridge that connects the two half cells in Exercise 38.Exercise 38 Sketch the following voltaic cell showing the
The nonspontaneous redox reaction of nickel and aqueous iron(II) sulfate is an electrolytic process according to the following equation. Ni(s) + FeSO4(aq) → Fe(s) + NiSO4(aq) The half-reactions
The nonspontaneous redox reaction of tin and aqueous cobalt(II) sulfate is an electrolytic process according to the following equation. Sn(s) + CoSO4(aq) → Co(s) + SnSO4(aq) The half-reactions
The nonspontaneous redox reaction of chlorine gas and aqueous sodium fluoride is an electrolytic process according to the following equation. Cl2(g) + 2 NaF(aq) → 2 NaCl(aq) + F2(g) The
The nonspontaneous redox reaction of bromine and aqueous sodium chloride is an electrolytic process according to the following equation. Br2(l) + 2 NaCl(aq) → 2 NaBr(aq) + Cl2(g)The half-reactions
Calculate the oxidation number for sulfur in sodium tetrathionate, Na2S4O6.
Calculate the oxidation number for sulfur in calcium thiosulfate, CaS2O3.
The redox reaction between cobalt metal and aqueous mercury(II) nitrate produces cobalt(II) nitrate and droplets of liquid mercury metal. Write a net ionic equation for the reaction.
The redox reaction between liquid mercury and aqueous gold(III) acetate produces mercury(I) acetate and gold metal. Write a net ionic equation for the reaction.
The redox reaction between zinc metal and sulfuric acid produces zinc sulfate and hydrogen gas. Write a net ionic equation for the reaction.
The redox reaction between aluminum metal and hydrochloric acid produces aluminum chloride and hydrogen gas. Write a net ionic equation for the reaction.
Write a balanced equation for the reaction of a copper penny in a dilute nitric acid solution. Cu(s) + NO3–(aq) → Cu2+(aq) + NO(g)
Write a balanced equation for the reaction of ethyl alcohol, C2H5OH, and an acidic potassium dichromate solution, which occurs in a “breathalyzer.” C2H5OH(aq) + Cr2O7 2–(aq) → HC2H3O2(aq) +
Which type of nuclear radiation is powerful light energy that is not deflected as it passes between electrically charged plates?(a) Alpha(b) Beta(c) Gamma(d) All of the above(e) None of the
Write a balanced nuclear equation for each of the following radioactive decay reactions.(a) Radon-222 decays by alpha and gamma emission.(b) Barium-133 decays by electron capture.
Identify nuclide X in the following nuclear reactions that represents the radioactive decay product from(a) Beta emission and(b) Positron emission. 99 43 (a) Tc (b) P 30 15 0 X + e → 4X + 0 +16

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