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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) H₂S (aq) + CO3²-(aq)→→ (b) HCN(aq) +
Heating a metal carbonate leads to decomposition.Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left, or (iii) shifts right.(a) Add
Carbonyl bromide decomposes to carbon monoxide and bromine.Kc is 0.190 at 73°C. Suppose you place 0.500 mol of COBr2 in a 2.00-L flask and heat it to 73°C (see Study Question 17). After equilibrium
Phosphorus pentachloride decomposes at elevated temperatures.An equilibrium mixture at some temperature consists of 3.120 g of PCl5, 3.845 g of PCl3, and 1.787 g of Cl2 in a 10.0-L flask. If you add
Equal molar quantities of sodium hydroxide and sodium hydrogen phosphate (Na2HPO4) are mixed.(a) Write the balanced, net ionic equation for the acid–base reaction that can, in principle, occur.(b)
Ammonium hydrogen sulfide decomposes on heating.If Kp for this reaction is 0.11 at 25°C (when the partial pressures are measured in atmospheres), what is the total pressure in the flask at
Equal molar quantities of hydrochloric acid and sodium hypochlorite (NaClO) are mixed.(a) Write the balanced, net ionic equation for the acid–base reaction that can, in principle, occur.(b) Does
Equal molar quantities of acetic acid and sodium hydrogen phosphate (Na2HPO4) are mixed.(a) Write a balanced, net ionic equation for the acid–base reaction that can, in principle, occur.(b) Does
Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide if the salt is heated to a sufficiently high temperature.Some ammonium iodide is placed in a flask, which is then heated to
Equal molar quantities of ammonia and sodium dihydrogen phosphate (NaH2PO4) are mixed.(a) Write a balanced, net ionic equation for the acid–base reaction that can, in principle, occur.(b) Does the
The equilibrium reaction N2O4(g) ⇄ 2 NO2(g) has been thoroughly studied (Figure 15.7).(a) If the total pressure in a flask containing NO2 and N2O4 gas at 25°C is 1.50 atm and the value of Kp at
When solid ammonium carbamate sublimes, it dissociates completely into ammonia and carbon dioxide according to the following equation:At 25°C, experiment shows that the total pressure of the gases
A 0.015 M solution of hydrogen cyanate, HOCN, has a pH of 2.67.(a) What is the hydronium ion concentration in the solution?(b) What is the ionization constant, Ka, for the acid?
A 0.025 M solution of hydroxylamine has a pH of 9.11. What is the value of Kb for this weak base? H₂NOH(aq) + H₂O(€) H3NOH+ (aq) + OH-(aq)
A 0.10 M solution of chloroacetic acid, ClCH2CO2H, has a pH of 1.95. Calculate Ka for the acid.
In the gas phase, acetic acid exists as an equilibrium of monomer and dimer molecules. (The dimer consists of two molecules linked through hydrogen bonds.)The equilibrium constant, Kc, at 25°C for
Methylamine, CH3NH2, is a weak base.If the pH of a 0.065 M solution of the amine is 11.70, what is the value of Kb? CH3NH₂(aq) + H₂O(l) CH3NH3+ (aq) + OH-(aq)
Assume 3.60 mol of ammonia is placed in a 2.00-L vessel and allowed to decompose to the elements at 723 K.If the experimental value of Kc is 6.3 for this reaction at the temperature in the reactor,
The total pressure for a mixture of N2O4 and NO2 is 0.15 atm. If Kp = 7.1 (at 25°C), calculate the partial pressure of each gas in the mixture. 2 NO₂(g) → N₂O4(g)
Kc for the decomposition of ammonium hydrogen sulfide is 1.8 × 10−4 at 25°C.(a) When the pure salt decomposes in a flask, what are the equilibrium concentrations of NH3 and H2S?(b) If NH4HS is
A 2.5 × 10−3 M solution of an unknown acid has a pH of 3.80 at 25°C.(a) What is the hydronium ion concentration of the solution?(b) Is the acid a strong acid, a moderately weak acid (Ka of about
A 0.015 M solution of a base has a pH of 10.09.(a) What are the hydronium and hydroxide ion concentrations of this solution?(b) Is the base a strong base, a moderately weak base (Kb of about 10−5),
COCl2 decomposes to CO and Cl2 at high temperatures. Kc at 600 K for the reaction is 0.0071.If 0.050 mol of COCl2 is placed in a 12.5-L flask, what is the total pressure at equilibrium at 600 K?
What are the equilibrium concentrations of hydronium ion, acetate ion, and acetic acid in a 0.20 M aqueous solution of acetic acid?
The ionization constant of a very weak acid, HA, is 4.0 × 10−9. Calculate the equilibrium concentrations of H3O+, A−, and HA in a 0.040 M solution of the acid.
A 15-L flask at 300 K contains 6.44 g of a mixture of NO2 and N2O4 in equilibrium. What is the total pressure in the flask? (Kp for 2 NO2 (g) ⇄ N2O4(g) is 7.1.)
Phenol (C6H5OH), commonly called carbolic acid, is a weak organic acid.If you dissolve 0.195 g of the acid in enough water to make 125 mL of solution, what is the equilibrium hydronium ion
What are the equilibrium concentrations of H3O+, CN−, and HCN in a 0.025 M solution of HCN? What is the pH of the solution?
Sulfuryl chloride, SO2Cl2, is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO2 and Cl2.(a) A 10.0-L flask containing 6.70
What are the equilibrium concentrations of NH3, NH4+, and OH− in a 0.15 M solution of ammonia? What is the pH of the solution?
The reaction of hydrogen and iodine to give hydrogen iodide has an equilibrium constant, Kc, of 56 at 435°C.(a) What is the value of Kp?(b) Suppose you mix 0.045 mol of H2 and 0.045 mol of I2 in a
The weak base methylamine, CH3NH2, has Kb = 4.2 × 10−4. It reacts with water according to the equationCalculate the equilibrium hydroxide ion concentration in a 0.25 M solution of the base. What
Limestone decomposes at high temperatures.At 1000°C, Kp = 3.87. If pure CaCO3 is placed in a 5.00-L flask and heated to 1000°C, what quantity of CaCO3 must decompose to achieve the equilibrium
A hypothetical weak base has Kb = 5.0 × 10−4. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH− in a 0.15 M solution of the base.
Hemoglobin (Hb) can form a complex with both O2 and CO. For the reactionat body temperature, K is about 200. If the ratio [HbCO]/[HbO2] comes close to 1, death is probable. What partial pressure of
Calculate the pH of a 0.12 M aqueous solution of the base aniline, C6H5NH2 (Kb = 4.0 × 10−10). CoH5NHz(aq) +H,O(l)< C6H5NH3+ (aq) + OH-(aq)
Explain why each of the following statements is incorrect.(a) Entropy increases in all spontaneous reactions.(b) Reactions with a negative free energy change (ΔrG° < 0) are product-favored and
Decide whether each of the following statements is true or false. If false, rewrite it to make it true.(a) The entropy of a substance increases on going from the liquid to the vapor state at any
Under what conditions is the entropy of a pure substance 0 J/K ∙ mol? Could a substance at standard conditions at 25°C have a value of 0 J/K ∙mol? A negative entropy value? Are there any
Iodine, I2, is much more soluble in an aqueous solution of potassium iodide, KI, than it is in pure water. The anion found in solution is I3−.(a) Draw an electron dot structure for I3−.(b) Write
Wet limestone is used to scrub SO2 gas from the exhaust gases of power plants. One possible reaction gives hydrated calcium sulfite:Another reaction gives hydrated calcium sulfate:(a) Which reaction
Sulfur undergoes a phase transition between 80 and 100°C.S8(rhombic) → S8(monoclinic)Δr H° = 3.213 kJ/mol-rxn Δr S° = 8.7 J/K ∙ mol-rxn(a) Estimate ΔrG° for the transition at 80.0°C and
Calculate the entropy change for dissolving HCl gas in water at 25°C. Is the sign of Δr S° what you expected? Why or why not?
Some metal oxides can be decomposed to the metal and oxygen under reasonable conditions. Is the decomposition of silver(I) oxide product favored at equilibrium at 25°C?2 Ag2O(s) → 4 Ag(s) +
Copper(II) oxide, CuO, can be reduced to copper metal with hydrogen at higher temperatures.CuO(s) + H2(g) → Cu(s) + H2O(g)Is this reaction product- or reactant-favored at equilibrium at 298 K?
Calculate Δf G° for HI(g) at 350°C, given the following equilibrium partial pressures: P(H2) =0.132 bar, P(I2) = 0.295 bar, and P(HI) = 1.61 bar.At 350°C and 1 bar, I2 is a gas.1⁄2 H2(g) +
Calculate the equilibrium constant for the formation of NiO at 1627°C. Can the reaction proceed in the forward direction if the initial pressure of O2 is below 1.00 mm Hg?{Δf G°[NiO(s)] =−72.1
Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature.TiO2(s) + 3 C(s) → 2 CO(g) + TiC(s)(a) Calculate ΔrG° and K at 727°C.(b) Is the reaction product-favored at
Cisplatin [cis-diamminedichloroplatinum(II)] is a potent treatment for certain types of cancers, but the trans isomer is not effective. What is the equilibrium constant at 298 K for the
Consider the formation of NO(g) from its elements. N2(g) + O2(g) ⇄ 2 NO(g)(a) Calculate Kp at 25°C. Is the reaction product favored at equilibrium at this temperature?(b) Assuming Δr H° and Δr
Write a chemical equation for the oxidation of C2H6(g) by O2(g) to form CO2(g) and H2O(g). Defining this as the system:(a) Predict whether the signs of ΔS°(system), ΔS°(surroundings), and
The normal melting point of benzene, C6H6, is 5.5°C. For the process of melting, what is the sign of each of the following?(a) Δr H°(b) Δr S°(c) ΔrG° at 5.5°C(d) ΔrG° at 0.0°C(e) ΔrG° at
Calculate the standard molar entropy change, Δr S°, for each of the following reactions at 25°C:(a) C(s) + 2 H2(g) → CH4(g)(b) CH4(g) + 1⁄2 O2(g) → CH3OH(ℓ)(c) C(s) + 2 H2(g) + 1⁄2 O2(g)
For each of the following processes, predict the algebraic sign of Δr H°, Δr S°, and ΔrG°. No calculations are necessary; use your common sense.(a) The decomposition of liquid water to give
“Heater Meals” are food packages that contain their own heat source. Just pour water into the heater unit, wait a few minutes, and voilà! You have a hot meal.(a) Confirm that this is a
Oxygen dissolved in water can cause corrosion in hot-water heating systems. To remove oxygen, hydrazine (N2H4) is often added. Hydrazine reacts with dissolved O2 to form water and N2.(a) Write a
Use values of Δf G° for solid and gaseous iodine at 25°C (Appendix L) to calculate the equilibrium vapor pressure of iodine at this temperature.Data given in Appendix L ⒸCengage Learning/Chades
The formation of diamond from graphite is a process of considerable importance.(a) Using data in Appendix L, calculate Δr S°, Δr H°, and ΔrG° for this process at 25°C.(b) The calculations will
Iodine, I2, dissolves readily in carbon tetrachloride. For this process, ΔH° = 0 kJ/mol. I2(s) → I2 (in CCl4 solution).What is the sign of ΔrG°? Is the dissolving process entropy-driven or
Write an equation for the reaction of Fe2O3(s) and C(s) to give Fe(s) and CO(g) (one of the reactions occurring in a blast furnace). How does ΔrG° vary with temperature? Is there a temperature at
Write an equation for the decomposition of 1.0 mol of gaseous methanol to the elements in their standard states.(a) How does the value of ΔrG° change as the temperature increases?(b) Is there a
The Haber–Bosch process for the production of ammonia is one of the key industrial processes in developed countries.N2(g) + 3 H2(g) ⇄ 2 NH3(g)(a) Calculate ΔrG° for the reaction at 298 K, 800
Consider the reaction of NO and Cl2 to produce NOCl.(a) What is ΔS°(system) for this reaction?(b) Does ΔS°(system) change with temperature?(c) Does ΔS°(surroundings) change with temperature?(d)
Two processes that can be used to generate hydrogen are the electrolysis of water 2 H2O(ℓ) → 2 H2(g) + O2(g) and the reaction of methane with steam CH4(g) + H2O(g) → 3 H2(g) + CO(g)(a)
Muscle cells need energy to contract. One biochemical pathway for energy transfer is the breakdown of glucose to pyruvate in a process called glycolysis. In the presence of sufficient oxygen in the
Hydrogen and methane are two possible replacements for gasoline in automobiles. The reactions for their combustion are as follows:H2(g)+ 1⁄2 O2(g) → H2O(ℓ)CH4(g) + 2 O2(g) → CO2(g) + 2
Determine if each of the following statements is true or false.(a) For a reaction that can yield more than one product, the most stable product is always formed in the greatest amount.(b) For a
Write balanced equations for the following half-reactions. Specify whether each is an oxidation or reduction.(a) Cr(s) → Cr3+(aq) (in acid)(b) AsH3(g) → As(s) (in acid)(c) VO3−(aq) → V2+(aq)
Write balanced equations for the following half-reactions. Specify whether each is an oxidation or reduction.(a) H2O2(aq) → O2(g) (in acid)(b) H2C2O4(aq) → CO2(g) (in acid)(c) NO3−(aq) →
Balance the following redox equations. All occur in acid solution.(a) Ag(s) + NO3−(aq) → NO2(g) + Ag+(aq)(b) MnO4−(aq) + HSO3−(aq) → Mn2+(aq) + SO42−(aq)(c) Zn(s) + NO3−(aq) →
Balance the following redox equations. All occur in acid solution.(a) Sn(s) + H+(aq) → Sn2+(aq) + H2(g)(b) Cr2O72−(aq) + Fe2+(aq) → Cr3+(aq) + Fe3+(aq)(c) MnO2(s) + Cl−(aq) → Mn2+(aq) +
Balance the following redox equations. All occur in basic solution.(a) Al(s) + H2O(ℓ) → Al(OH)4−(aq) + H2(g)(b) CrO42−(aq) + SO32−(aq) → Cr(OH)3(s) + SO42−(aq)(c) Zn(s) + Cu(OH)2(s) →
A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions.Complete the following sentences: Electrons in the external circuit flow from the _______ electrode to the _______
Balance the following redox equations. All occur in basic solution.(a) Fe(OH)3(s) + Cr(s) → Cr(OH)3(s) + Fe(OH)2(s)(b) NiO2(s) + Zn(s) → Ni(OH)2(s) + Zn(OH)2(s)(c) Fe(OH)2(s) + CrO42−(aq) →
A voltaic cell is constructed using the reaction(a) Write equations for the oxidation and reduction half-reactions.(b) Which half-reaction occurs in the anode compartment, and which occurs in the
The half-cells Fe2+(aq) | Fe(s) and O2(g) | H2O (in acid solution) are linked to create a voltaic cell.(a) Write equations for the oxidation and reduction half-reactions and for the overall (cell)
The half-cells Sn2+(aq) | Sn(s) and Cl2(g) | Cl−(aq) are linked to create a voltaic cell.(a) Write equations for the oxidation and reduction half-reactions and for the overall (cell) reaction.(b)
(a) Write a balanced chemical equation for the formation of 1 mol of MgO(s) from the elements in their standard states. (Find the value for ∆fH° for MgO(s) in Appendix L.) (b) What is the
Using spdf and noble gas notations, write electron configurations for atoms of the following elements. (Try to do this by looking at the periodic table but not at Table 7.3.)(a) Strontium, Sr. This
A solution of KMnO4 absorbs light at 540 nm (page 206). What is the frequency of the light absorbed? What is the energy of one mole of photons with λ = 540 nm?Data given on Page 206
Suppose hydrogen atoms absorb energy so that electrons are excited to the n = 7 energy level. Electrons then undergo these transitions, among others: (a) n = 7→ n = 1; (b) n = 7 → n = 6;
The rare earth elements, or lanthanides, commonly exist as 3+ ions. Using an orbital box diagram and noble gas notation, show the electron configurations of the following elements and ions.(a) Ce and
Which of the following is not an allowable set of quantum numbers? Explain your answer briefly. For those sets that are valid, identify an element in which an outermost valence electron could have
A possible excited state for the H atom has an electron in a 4p orbital. List all possible sets of quantum numbers (n, ℓ, mℓ, ms) for this electron.
The magnet in the following photo is made from neodymium, iron, and boron. (a) Write the electron configuration of each of these elements using an orbital box diagram and noble gas notation.(b) Are
Name the element corresponding to each characteristic below.(a) The element with the electron configuration 1s22s22p63s23p3(b) The alkaline earth element with the smallest atomic radius(c) The
Arrange the following atoms in order of increasing ionization energy: Si, K, P, and Ca.
Rank the following in order of increasing ionization energy: Cl, Ca2+, and Cl−. Briefly explain your answer.
Answer the questions below about the elements A and B, which have the electron configurations shown. A = [Kr]5s1 B = [Ar]3d104s24p4(a) Is element A a metal, nonmetal, or metalloid? (b) Which
Answer the following questions about the elements with the electron configurations shown here: A = [Ar]4s2 B = [Ar]3d104s24p5(a) Is element A a metal, metalloid, or nonmetal?(b) Is element B a
Which of the following ions are unlikely to be found in a chemical compound: Cs+, In4+, Fe6+, Te2−, Sn5+, and I−? Explain briefly.
Place the following ions in order of decreasing size: K+, Cl−, S2−, and Ca2+.
Answer each of the following questions: (a) Of the elements S, Se, and Cl, which has the largest atomic radius?(b) Which has the larger radius, Br or Br−?(c) Which should have the largest
The following are isoelectronic species: Cl−, K+, and Ca2+. Rank them in order of increasing(a) Size,(b) Ionization energy, and(c) Electron attachment enthalpy
Compare the elements Na, B, Al, and C with regard to the following properties: (a) Which has the largest atomic radius? (b) Which has the most negative electron attachment enthalpy?(c) Place the
The configuration for an element is given here.(a) What is the identity of the element with this configuration?(b) Is a sample of the element paramagnetic or diamagnetic?(c) How many unpaired
Two elements in the second transition series (Y through Cd) have four unpaired electrons in their 3+ ions. What elements fit this description?
The configuration of an element is given here. (a) What is the identity of the element? (b) In what group and period is the element found? (c) Is the element a nonmetal, a main group element, a
Answer the questions below about the elements A and B, which have the ground state electron configurations shown(a) Is element A a metal, nonmetal, or metalloid? (b) Which element has the greater
What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3. Electron 1 2 3 1 2 [Kr] ↑↑↑↑ d orbitals n l 3 N s orbital me ms

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