A student ran the following reaction in the laboratory at 527 K: COCl2(g) CO(g) + Cl2(g)

When she introduced 1.60 moles of COCl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 1.57 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc =

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

a chemical change results in a new substance being formed; whereas a physical change will result in a different state of matter

explanation: