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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Indicate which of the following processes are reversible.(a) Nitrogen gas expands into a vacuum.(b) Dry ice, CO2(s), sublimes at 25°C and 1.0 atm.(c) Energy as heat is added to a mixture of ice and
Indicate which of the following processes are reversible.(a) Nitrogen and oxygen gases diffuse to give a homogeneous mixture.(b) Ice sublimes at −5°C and 1.0 atm.(c) Energy as heat is transferred
What information is needed to calculate the entropy change that occurs when 1.00 mole of water vapor condenses to liquid water at 100°C?
What information is needed to calculate the entropy change when a 2.25 g sample of liquid water is warmed from 20°C to 25°C?
Calculate the entropy change that occurs when 0.50 mol of ice is converted to liquid water at 0°C in a reversible process. (qfus = 333 J/g)
Calculate the entropy change that occurs when 1.00 mol of steam is converted to liquid water at 100°C in a reversible process. (qvap = 40. 7 kJ/mol)
Calculate the change in entropy for a system in going from a condition of 5 accessible microstates to 30 accessible microstates.
Calculate the change in entropy of a system with an increase in volume from 1.0 L to 2.0 L.
The third law of thermodynamics says that a perfect crystal at 0 K has zero entropy. The standard entropy of a substance, S° can be determined by evaluating the energy required to carry out
Identify trends in S° values:(a) For the halogens: F2(g), Cl2(g), Br2(ℓ), I2(s).(b) For the gaseous hydrocarbons: CH4, C2H6, C3H8.
Which substance has the higher entropy?(a) Dry ice (solid CO2) at −78°C or CO2(g) at 0°C(b) Liquid water at 25°C or liquid water at 50°C(c) Pure alumina, Al2O3(s), or ruby (ruby is Al2O3 in
Which substance has the higher entropy?(a) A sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus(b) O2(g) at
Use S° values to calculate the standard entropy change, ΔrS°, for each of the following processes and comment on the sign of the change.(a) KOH(s) → KOH(aq)(b) Na(g) → Na(s)(c) Br2(ℓ) →
Use S° values to calculate the standard entropy change, ΔrS°, for each of the following processes, and comment on the sign of the change.(a) NH4Cl(s) → NH4Cl(aq)(b) CH3OH(ℓ) → CH3OH(g)(c)
Calculate the standard entropy change for the formation of 1.0 mol of the following compounds from the elements at 25°C.(a) HCl(g) (b) Ca(OH)2(s)
Calculate the standard entropy change for the formation of 1.0 mol of the following compounds from the elements at 25°C.(a) H2S(g)(b) MgCO3(s)
Calculate the standard entropy change for the following reactions at 25°C. Comment on the sign of Δr S°.(a) 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s)(b) 2 CH3OH(ℓ) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)
Calculate the standard entropy change for the following reactions at 25°C. Comment on the sign of Δr S°.(a) 2 Na(s) + 2 H2O(ℓ) → 2 NaOH(aq) + H2(g)(b) Na2CO3(s) + 2 HCl(aq) → 2 NaCl(aq)
Classify each of the reactions according to one of the four reaction types summarized in Table 18.1.Δr H° = −851.5 kJ/mol-rxnΔr S° = −375.2 J/K · mol-rxnΔr H° = 66.2 kJ/mol-rxnΔr S° =
Is the reaction Si(s) + 2 Cl2(g) → SiCl4(g) spontaneous under standard conditions at 298.15 K? Answer this question by calculating ΔS°(system), ΔS°(surroundings), and ΔS°(universe). (Define
Is the reaction Si(s) + 2 H2(g) → SiH4(g) spontaneous under standard conditions at 298.15 K? Answer this question by calculating ΔS°(system), ΔS°(surroundings), and ΔS°(universe). (Define
Calculate ΔS°(universe) for the decomposition of 1 mol of liquid water to form gaseous hydrogen and oxygen. Is this reaction spontaneous under standard conditions at 25°C? Explain your answer
Calculate ΔS°(universe) for the formation of 1 mol HCl(g) from gaseous hydrogen and chlorine. Is this reaction spontaneous under standard conditions at 25°C? Explain your answer briefly.
Classify each of the reactions according to one of the four reaction types summarized in Table 18.1.Δr H° = −673 kJ/mol-rxnΔr S° = 60.4 J/K · mol-rxnΔr H° = 490.7 kJ/mol-rxnΔr S° = 197.9
Using values of Δf H° and S°, calculate ΔrG° for each of the following reactions at 25°C.(a) 2 Pb(s) + O2(g) → 2 PbO(s)(b) NH3(g) + HNO3(aq) → NH4NO3(aq)Which of these reactions is (are)
Using values of Δf H° and S°, calculate ΔrG° for each of the following reactions at 25°C.(a) 2 Na(s) + 2 H2O(ℓ) → 2 NaOH(aq) + H2(g)(b) 6 C(graphite) + 3 H2(g) → C6H6(ℓ)Which of these
Using values of Δf H° and S°, calculate the standard molar free energy of formation, Δf G°, for each of the following compounds:(a) CS2(g)(b) NaOH(s)(c) ICl(g)Compare your calculated values of
Using values of Δf H° and S°, calculate the standard molar free energy of formation, Δf G°, for each of the following:(a) Ca(OH)2(s)(b) Cl(g)(c) Na2CO3(s)Compare your calculated values of Δf
For the reaction BaCO3(s) → BaO(s) + CO2(g), ΔrG° = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of Δf G° for BaCO3(s).Data given in Appendix
For the reaction TiCl2(s) + Cl2(g) → TiCl4(ℓ),ΔrG° = −272.8 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of Δf G° for TiCl2(s).Data given in
Determine whether the reactions listed below are entropy-favored or disfavored under standard conditions. Predict how an increase in temperature will affect the value of ΔrG°.(a) N2(g) + 2 O2(g)
Determine whether the reactions listed below are entropy-favored or disfavored under standard conditions. Predict how an increase in temperature will affect the value of ΔrG°.(a) I2(g) → 2
Heating some metal carbonates, among them magnesium carbonate, leads to their decomposition.(a) Calculate ΔrG° and Δr S° for the reaction.(b) Is the reaction product-favored at equilibrium at 298
Calculate Δr H° and Δr S° for the reaction of tin(IV) oxide with carbon.(a) Is the reaction product-favored at equilibrium at 298 K?(b) Is the reaction predicted to be product-favored at
The ionization constant, Ka, for acetic acid is 1.8 ×10–5 at 25°C. What is the value of ΔrG° for this reaction? Is this reaction product- or reactant favored at equilibrium?
Using values of Δf G°, calculate ΔrG° for each of the following reactions at 25°C. Which are product-favored at equilibrium?(a) 2 K(s) + Cl2(g) → 2 KCl(s)(b) 2 CuO(s) → 2 Cu(s) + O2(g)(c) 4
Using values of Δf G°, calculate ΔrG° for each of the following reactions at 25°C. Which are product favored at equilibrium?(a) HgS(s) + O2(g) → Hg(ℓ) + SO2(g)(b) 2 H2S(g) + 3 O2(g) → 2
The formation constant, Kf, for the reactionis 1.1 × 107. What is the value of ΔrG° for this reaction? Is the reaction product- or reactant-favored at equilibrium? Ag+(aq) + 2 NH
The standard free energy change, ΔrG°, for the formation of NO(g) from its elements is +86.58 kJ/mol-rxn at 25°C. Calculate Kp at this temperature for the equilibriumComment on the sign of ΔrG°
The standard free energy change, ΔrG°, for the formation of O3(g) from O2(g) is +163.2 kJ/mol-rxn at 25°C. Calculate Kp at this temperature for the equilibriumComment on the sign of ΔrG° and the
Calculate ΔrG° at 25°C for the formation of 1.00 mol of C2H6(g) from C2H4(g) and H2(g). Use this value to calculate Kp for the equilibrium.Comment on the sign of ΔrG° and the magnitude of Kp.
Calculate ΔrG° at 25°C for the formation of 1.00 mol of C2H5OH(g) from C2H4(g) and H2O(g). Use this value to calculate Kp for the equilibrium.Comment on the sign of ΔrG° and the magnitude of Kp.
For the synthesis of ammonia from its elements at 25°C,N2(g) + 3 H2(g) → 2 NH3(g)(a) Calculate ΔrG°using values of Δf G°. Is the reaction product-favored at equilibrium?(b) Calculate ΔrG when
For the decomposition of solid calcium carbonate at 25°C,(a) Calculate ΔrG° using values of Δf G°. Is the reaction product-favored at equilibrium?(b) Calculate ΔrG when the partial pressure of
Compare the compounds in each set below and decide which is expected to have the higher entropy. Assume all are at the same temperature. Check your answers using data in Appendix L.(a) HF(g), HCl(g),
Using standard entropy values, calculate Δr S° for the formation of 1.0 mol of NH3(g) from N2(g) and H2(g) at 25°C.
About 5 billion kilograms of benzene, C6H6, are made each year. Benzene is used as a starting material for many other compounds and as a solvent (although it is also a carcinogen, and its use is
Hydrogenation, the addition of hydrogen to an organic compound, is an industrially important reaction. Calculate Δr H°, Δr S°, and ΔrG° for the hydrogenation of octene, C8H16, to give octane,
Is the combustion of ethane, C2H6, product-favored at equilibrium at 25°C?C2H6(g) + 7⁄2 O2(g) → 2 CO2(g) + 3 H2O(g)Answer the question by calculating the value of ΔS°(universe) at 298 K, using
When vapors from hydrochloric acid and aqueous ammonia come in contact, they react, producing a white “cloud” of solid NH4Cl (Figure 18.9). HCl(g) + NH3(g) ⇄ NH4Cl(s)Defining the reactants and
Write a balanced equation that depicts the formation of 1 mol of Fe2O3(s) from its elements. What is the standard free energy of formation of 1.00 mol of Fe2O3(s)? What is the value of ΔG° when 454
Calculate ΔS°(system), ΔS°(surroundings), and ΔS°(universe) for each of the following processes at 298 K, and comment on how these systems differ.(a) HNO3(g) → HNO3(aq)(b) NaOH(s) → NaOH(aq)
Methanol is now widely used as a fuel in race cars. Consider the following reaction as a possible synthetic route to methanol.C(graphite) + 1⁄2 O2(g) + 2 H2(g) ⇄ CH3OH(ℓ)Calculate Kp for the
The enthalpy of vaporization of liquid diethyl ether, (C2H5)2O, is 26.0 kJ/mol at the boiling point of 35.0°C. Calculate ΔS° for a vapor-to-liquid transformation at 35.0°C.
Calculate the entropy change, Δr S°, for the vaporization of ethanol, C2H5OH, at its normal boiling point, 78.0°C. The enthalpy of vaporization of ethanol is 39.3 kJ/mol.
Using thermodynamic data, estimate the normal boiling point of ethanol. (Recall that liquid and vapor are in equilibrium at 1.0 atm pressure at the normal boiling point.) The actual normal boiling
The following reaction is reactant-favored at equilibrium at room temperature.COCl2(g) → CO(g) + Cl2(g)Will raising or lowering the temperature make it product favored?
Yeast can produce ethanol by the fermentation of glucose (C6H12O6), which is the basis for the production of most alcoholic beverages.C6H12O6(aq) → 2 C2H5OH(ℓ) + 2 CO2(g)Calculate Δr H°, Δr
When calcium carbonate is heated strongly, CO2 gas is evolved. The equilibrium pressure of CO2 is 1.00 bar at 897°C, and Δr H° at 298 K is 179.0 kJ/mol-rxn.CaCO3(s) → CaO(s) + CO2(g)Estimate the
Sodium reacts violently with water according to the equation Na(s) + H2O(ℓ) → NaOH(aq) + 1⁄2 H2(g) Without doing calculations, predict the signs of Δr H° and Δr S° for the reaction. Verify
The equilibrium constant, Kp, for N2O4(g) ⇄ 2 NO2(g) is 0.14 at 25°C. Calculate ΔrG° for the conversion of N2O4(g) to NO2(g) from this constant, and compare this value with that determined from
Elemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2.BCl3(g) + 3⁄2 H2(g) → B(s) + 3 HCl(g)Calculate Δr H°, Δr S°, and ΔrG° at 25°C for this reaction.
Estimate the vapor pressure of ethanol at 37°C using thermodynamic data. Express the result in millimeters of mercury.
The equilibrium constant for the butane ⇄ isobutane equilibrium at 25°C is 2.50. Calculate ΔrG° at this temperature in units of kJ/mol. isobutane CH3 CH,CH,CH,CH, <
Estimate the boiling point of water in Denver, Colorado (where the altitude is 1.60 km and the atmospheric pressure is 630 mm Hg or 0.840 bar).
A crucial reaction for the production of synthetic fuels is the production of H2 by the reaction of coal with steam. The chemical reaction is C(s) + H2O(g) → CO(g) + H2(g)(a) Calculate ΔrG° for
Calculate ΔrG° for the decomposition of sulfur trioxide to sulfur dioxide and oxygen.2 SO3(g) ⇄ 2 SO2(g) + O2(g)(a) Is the reaction product-favored at equilibrium at 25°C?(b) If the reaction is
Methanol can be made by partial oxidation of methane by O2(g).CH4(g) + 1⁄2 O2(g) ⇄ CH3OH(ℓ)(a) Determine ΔS°(system), ΔS°(surroundings), and ΔS°(universe) for this process.(b) Is this
A cave in Mexico was recently discovered to have some interesting chemistry. Hydrogen sulfide, H2S, reacts with oxygen in the cave to give sulfuric acid, which drips from the ceiling in droplets with
Draw a Lewis structure for each of the following molecules or ions:(a) BrF5(b) IF3(c) IBr2−(d) BrF2+
Determine the formal charge on each atom in the following molecules or ions:(a) N2H4(b) PO43−(c) BH4−(d) NH2OH
Determine the formal charge on each atom in the following molecules or ions:(a) SCO(b) HCO2− (formate ion)(c) CO32−(d) HCO2H (formic acid)
Determine the formal charge on each atom in the following molecules and ions:(a) NO2+(b) NO2−(c) NF3(d) HNO3
Determine the formal charge on each atom in the following molecules and ions:(a) SO2(b) OSCl2(c) O2SCl2(d) FSO3−
Draw a Lewis structure for each of the following molecules or ions. Describe the electron-pair geometry and molecular geometry around the central atom.(a) NH2Cl(b) Cl2O (O is the central atom)(c)
Draw a Lewis structure for each of the following molecules or ions. Describe the electron-pair geometry and molecular geometry around the central atom.(a) ClF2+(b) SnCl3−(c) PO43−(d) CS2
The following molecules or ions all have two oxygen atoms attached to a central atom. Draw a Lewis structure for each one, and then describe the electron-pair geometry and molecular geometry around
Give approximate values for the indicated bond angles.(a) O—S—O angle in SO2(b) F—B—F angle in BF3(c) Cl—C—Cl angle in Cl2CO(d) H—C—H (angle 1) and C—C≡N (angle 2) in acetonitrile
The following molecules or ions all have three oxygen atoms attached to a central atom. Draw a Lewis structure for each one, and then describe the electron-pair geometry and molecular geometry around
Draw a Lewis structure for each of the following molecules or ions. Describe the electron-pair geometry and molecular geometry around the central atom.(a) ClF2−(b) ClF3(c) ClF4−(d) ClF5
Give approximate values for the indicated bond angles:(a) Cl—S—Cl in SCl2(b) N—N—O in N2O(c) Bond angles 1, 2, and 3 in vinyl alcohol (a component of polymers and a molecule found in outer
Draw a Lewis structure for each of the following molecules or ions. Describe the electron-pair geometry and molecular geometry around the central atom.(a) SiF62−(b) PF5(c) SF4(d) XeF4
Phenylalanine is one of the natural amino acids and is a “breakdown” product of the artificial sweetener aspartame. Estimate the values of the indicated angles in the amino acid. Explain why the
Acetylacetone has the structure shown here. Estimate the values of the indicated angles. H H₂C C C- 2 1:0: H C-CH₂ :0:-3 1 Acetylacetone 2 3
For each pair of bonds, indicate the more polar bond, and use an arrow to show the direction of polarity in each bond.(a) C—O and C—N(b) P—Br and P—Cl(c) B—O and B—S(d) B—F and B—I
Acrolein, C3H4O, is the starting material for certain plastics.(a) Which bonds in the molecule are polar, and which are nonpolar?(b) Which is the most polar bond in the molecule? Which is the more
Urea, (NH2)2CO, is used in plastics and fertilizers. It is also the primary nitrogen-containing substance excreted by humans.(a) Which bonds in the molecule are polar, and which are nonpolar?(b)
For each of the bonds listed below, tell which atom is the more negatively charged.(a) C—N(b) C—H(c) C—Br(d) S—O
Considering both formal charges and bond polarities, predict on which atom or atoms the negative charge resides in the following anions:(a) OH−(b) BH4−(c) CH3CO2−
Considering both formal charge and bond polarities, predict on which atom or atoms the positive charge resides in the following cations:(a) H3O+(b) NH4+(c) NO2+(d) NF4+
Three resonance structures are possible for dinitrogen monoxide, N2O.(a) Draw the three resonance structures.(b) Calculate the formal charge on each atom in each resonance structure.(c) Based on
Three resonance structures are possible for the thiocyanate ion, SCN−.(a) Draw the three resonance structures.(b) Calculate the formal charge on each atom in each resonance structure.(c) Based on
Compare the electron dot structures of the hydrogen carbonate ion and nitric acid.(a) Are these species isoelectronic?(b) How many resonance structures does each species have?(c) What are the formal
Compare the electron dot structures of the carbonate (CO32−) and borate (BO33−) ions.(a) Are these ions isoelectronic?(b) How many resonance structures does each ion have?(c) What are the formal
The chemistry of the nitrite ion and HNO2:(a) Two resonance structures are possible for NO2−. Draw these structures, and then find the formal charge on each atom in each resonance structure.(b) In
Draw the resonance structures for the formate ion, HCO2−, and find the formal charge on each atom. If an H+ ion is attached to HCO2− (to form formic acid), does it attach to C or O?
Consider the following molecules:(a) H2O(b) NH3(c) CO2(d) ClF(e) CCl4(i) In which compound are the bonds most polar?(ii) Which compounds in the list are not polar?(iii) Which atom in ClF is more
Which of the following molecules is(are) polar? For each polar molecule, indicate the direction of polarity—that is, which is the negative end, and which is the positive end of the molecule.(a)
Which of the following molecules is(are) not polar? For each polar molecule, indicate the direction of polarity—that is, which is the negative end and which is the positive end.(a) BCl3(b) CF4(c)
Give the bond order for each bond in the followingmolecules or ions:(a) CH2O(b) SO32−(c) NO2+(d) NOCl

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