Use standard reduction potentials to find the equilibrium constant for the following reaction at 25°C: 2Ce4+(aq) + 2Cl−(aq) ⇌ 2Ce3+(aq) + Cl2(g) Enter your answer in scientific notation to one significant digit.

The equilibrium constant for the following reaction = 501.18

Explanation:

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally