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Given: Delta G = Delta G degree + RT In Q With respect to this equation, which of the following statements is NOT correct? Delta G = 0 is the condition for equilibrium. At equilibrium, Q becomes K. If Q = 1, then Delta G must equal Delta G degree. Delta G degree = 0 is the condition for equilibrium. What is the new pH if 10.0 mL of .10 M HCl is added to 120. ml. of a buffer that is .10 M acetic acid and .10 M acetate, K_2 for acetic acid = 1.8 times 10^-5. 4.71 4.74 4.82 4.67 What is the mass (in g) of silver chromate (MW = 331.7 g/mol) that can dissolve in 1.00 I. of 0.10 M AgNO_3 solution? The solubility product for Ag_2CrO_4: K_sp = 1.2 times 10^-2 7.96 times 10^-9 g 3.98 times 10^-9 g 3.98 times 10^-8 g 1.99 times 10^-8 g What is the total number (n) of e transferred in the following redox equation: 14 H^+ Cr_2O_7^2 + 6 Fe^2+ rightarrow 6Fe^3+ + 2Cr^3+ +7 H_2O n=1 n=3 n=6 n=12 Given 2 Al degree (s) + 3 Cd^2+ (aq) rightarrow 2 Al^3+ (aq) + 3Cd degree (s) For this reaction E degree = 1.26 v. If [Al^3+] = 0.01 M and [Cd^2+] = 10^-4 M. Calculate E from the Nernst equation: E = E_0 - .0257/n In Q 1.34 v 1.26 v 1.18 v 1.21 v
Given: Delta G = Delta G degree + RT In Q With respect to this equation, which of the following statements is NOT correct? Delta G = 0 is the condition for equilibrium. At equilibrium, Q becomes K. If Q = 1, then Delta G must equal Delta G degree. Delta G degree = 0 is the condition for equilibrium. What is the new pH if 10.0 mL of .10 M HCl is added to 120. ml. of a buffer that is .10 M acetic acid and .10 M acetate, K_2 for acetic acid = 1.8 times 10^-5. 4.71 4.74 4.82 4.67 What is the mass (in g) of silver chromate (MW = 331.7 g/mol) that can dissolve in 1.00 I. of 0.10 M AgNO_3 solution? The solubility product for Ag_2CrO_4: K_sp = 1.2 times 10^-2 7.96 times 10^-9 g 3.98 times 10^-9 g 3.98 times 10^-8 g 1.99 times 10^-8 g What is the total number (n) of e transferred in the following redox equation: 14 H^+ Cr_2O_7^2 + 6 Fe^2+ rightarrow 6Fe^3+ + 2Cr^3+ +7 H_2O n=1 n=3 n=6 n=12 Given 2 Al degree (s) + 3 Cd^2+ (aq) rightarrow 2 Al^3+ (aq) + 3Cd degree (s) For this reaction E degree = 1.26 v. If [Al^3+] = 0.01 M and [Cd^2+] = 10^-4 M. Calculate E from the Nernst equation: E = E_0 - .0257/n In Q 1.34 v 1.26 v 1.18 v 1.21 v
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