Use the halt-reaction method to balance each of the following in basic solution
a.
b.
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- Calculate the value of E for each of the following reactions. Decide whether each is product-favored at equilibrium in the direction written. [Reaction (d) is carried out in basic solution.] (a) Br2() + Mg(s) Mg2+(aq) + 2 Br(aq) (b) Zn2+(aq) + Mg(s) Zn(s) + Mg2+(aq) (c) Sn2+(aq) + 2 Ag+(aq) Sn4+(aq) + 2Ag(s) (d) 2 Zn(s) + O2(g) + 2 H2O() + 4 OH(aq) 2[Zn(OH)4]2(aq)arrow_forwardCalculate rG and the equilibrium constant for the following reactions. (a) 2 Fe3+(aq) + 2 I(aq) 2 Fe2+(aq) + I2(aq) (b) I2(aq) + 2 Br(aq) 2 I(aq) + Br2()arrow_forwardSome calculators cannot display results of an antilog calculation if the power of 10 is greater than 99. This shortcoming can come into play for determining equilibrium constants of redox reactions, which are sometimes quite large. Solve the following expressions for K: (a) logK=45.63 , (b) logK=25.00 , (c) logK=20.63 . is the relationship among the three expressions and the three answers? How can you use this relationship to solve problems that exceed 1099 even if your calculator will not carry out the calculation directly?arrow_forward
- The thermite reaction is 2Al(s) + Fe2O3(s) Al2O3(s) + 2Fe(s) (a) Calculate G for this reaction. (b) Calculate Keq for this reaction. Assume T = 298 K. You may have to do some mathematical manipulations to get your final numerical answer.arrow_forward12.19 For each of the following equations, write the equilibrium expression for the reverse reaction. 2C(s) + O,(g)^2CO(g) AgCl(s)5=BAg+(aq) + Crarrow_forwardAssume 25oC in all equilibria calculations. Express your answers in four decimal places. Do not use rounded-off values in subsequent calculations. Consider the dissociation reaction in 0.2103 M aqueous solution of HNO2 (Ka = 4.0 x 10-4): HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO2-(aq) Calculate the following: a. [HNO2] = b. %ionization =arrow_forward
- 50 mL 0.1 M A(NO3)2 , 100 mL 0.1 M NaCl , 100 mL 0.1 M ACl4-2 solutions are mixed. Determine the direction in which reaction proceeds. ( Kc = 5,5*105 )arrow_forwardFor the reaction below, Kc = 9.2 × 10⁻⁵. What is the equilibrium concentration of D if the reaction begins with 0.80 M A? A (aq) + 2 B (s) ⇌ C (s) + 2 D (aq)arrow_forward1. Predict in which direction (toward the products side or toward the reactants side) that each of the following redox reactionsproceeds under standard conditions. (a) Ni(s) + Zn2+(aq) → Ni2+(aq) + Zn(s) (b) Al(s) + 3 Ag + (aq) → Al3+(aq) + 3 Ag(s)arrow_forward
- Kc = 5.2 × 10⁻⁵ for the reaction below. What is the equilibrium concentration of D if the reaction begins with 0.20 M A? A (aq) + 2 B (s) ⇌ C (s) + 2 D (aq)arrow_forwardPredict whether the following reactions would occur spontaneously in aqueous solution at 25°C. Assume that the initial concentrations of dissolved species are all 1.0 M(a) Ca(s) + Cd2+(aq) → Ca2+(aq) + Cd(s)(b) 2Br¯ (aq) + Sn2+ (aq) → Br2(l) + Sn(s)(c) 2Ag(s) + Ni2+(aq) → 2Ag+(aq) + Ni(s)(d) Cu+(aq) + Fe3+(aq) → Cu2+(aq) + Fe2+(aq)arrow_forward2Ti2+ + Sn4+ ↔ 2Ti3+ + Sn2+ reaction Calculate the equilibrium constant. Sn4+ + 2e- ↔ Sn2+ , E0 = +0.54 V Ti3+ + e- ↔ Ti2+ , E0 = -0.369 Varrow_forward
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