Use the activity series in Table 15.3 to predict whether each of the following reactions will occur spontaneously:
a.
b.
c.
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Basic Chemistry
- 8) What is the pH of a solution containing 0.280 M weak base, B', with a K, of 3.9 X 107? (10.51) в (ад) + H-0 (1) ВН (аq) + ОН (ад)arrow_forward(Q55) Nickel carbonate is being precipitated out of a 1.00 L solution. If the concentration of dissolved nickel is 0.203, what mass (in micrograms) of sodium carbonate (Na2CO3) must be added for precipitation to begin? The Ksp of nickel carbonate is 1.42 x 107. 1 gram = 1 x 10 micrograms (ug)arrow_forward(7.12) A technician plates a faucet with 0.86 g Cr metal by electrolysis of aqueous Cr2(SO4)3. If 12.5 min is allowed for the plating, what current is needed? Molar mass of Cr: 51.996 g/mol Analysis/Strategy: mass of Cr ® mol Cr mol e¯ (or Faraday) ® coulombs ® amperes Reduction half-reaction of chromium solution to chromium metal: Cr* ,+3, (aq) e¯ ® Cr(s) + chromium solution, Cr2(SO4)3, has the ions: [Cr*3 s04-²] Answer: The current needed is ampere. (2 sig fig)arrow_forward
- (10) * Which reaction is an example of both a precipitation and a neutralization? (A) H3PO4(aq) + 3 KOH(aq) –→ K3PO4(aq) + 3 H2O(1) (B) FeC13(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCI(aq) (C) (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H20(1) (D) H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2 H2O(1) (E) 2 C(s) + 02(g) → 2 CO(g) (11) * All of the statements regarding redox reactions are true except (A) a reducing agent causes another substance to be reduced. (B) halogens usually behave as oxidizing agents because they readily gain electrons. (C) metal ions are produced when pure metals are oxidized. (D) when a substance is oxidized its charge (or oxidation number) decreases. (E) alkali metals often behave as reducing agents because they readily lose electrons. (12) In a typical oxidation-reduction reaction the electrons are transferred (A) from the oxidizing agent to the reducing agent. (B) from what is being oxidized to the substance being reduced. (C) from what is being reduced to the substance being…arrow_forward(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (aq) - Cro, (aq) + Clug Analysis: Balancing under acidic condition first (adding H30 & H*) Oxidation-Half reation: Balancing atoms & charges: Cr(OH)) * H20 - Cro, ug) + Reduction-Half reation: Balancing atoms and charges: e Clap H20 Balancing electrons lost & galned Multiply oxidation-half reaction by e's Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forward(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (nq) - Cro, (aq) Analysis: Balancing under acidic condition first (adding H30 & H") Oxidation-Half reation: Balancing atoms & charges: Cr(OH)x) * H20 - Cro, ug * H' + Reduction-Half reation: Balancing atoms and charges: 10 taq H20 Balancing electrons lost & gained Multiply oxidation-half reaction by Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forward
- 14.60 When iodine is oxidized in concentrated HNO3, it produces the white solid iodic acid, HIO3: L(s)+NO;(aq) HIO3(s)+NO2(g) Balance this equation, adding H*(aq) and H2O(1) as necessary.arrow_forward7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s) Sr2 (aq) 2F (aq) 2arrow_forwardGiven the following equilibrium constants at 433°C, 1 Na20(s) = 2 Na(1) +02 (9) K1 = 5 x 10-25 2 1 NaO(g) - Na(1)+;02(9) K2 8 x 10-5 -29 Na2 O2 (s) = 2 Na(1) + O2 (9) NaO2 (s) = Na(1) + O2 (9) K3 = 4 × 10 -14 KĄ 3 x 10 determine the values for the equilibrium constants for the following reactions: a. Na20(s) + 1 O2 (g) = Na2 O2 (8) Equilibrium constant = b. NaO(g) + Na, 0(s) = Na2O2(s) + Na(1) Equilibrium constant c. 2 NaO(g) = Na2 O2 (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)arrow_forward
- ■ 31. Consider the reaction A → 2 B. Initialy 1.5 mol of A is present and no B. What are the amounts of A and B when the extent of reaction is 0.60 mol? (.9, 1.2 mol) 21 10 mol the Gibbs energyarrow_forwardAt high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.arrow_forward(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + Clo (aq) - Cro, 2(aq) • Clzup Analysis: Balancing under acidic condition first (adding Hy0 & H") Oxidation-Half reation: Balancing atoms & charges: Cr(OH)y) * H20 - Cro, ng) + H' Reduction-Half reation: Balancing atoms and charges: CIo (aq) e Clp H20 Balancing electrons lost & gained Multiply oxidation-half reaction by e's Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forward
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