Use Le Chatelier’s principle to predict how the equilibrium concentration of the FeCl2+ ion will change when an aqueous solution of silver (I) nitrate, AgNO3, is added to the exothermic reaction below.
Fe3+(aq) + Cl-(aq) → FeCl2+(aq)
increase
decrease
no effect

d. temperate deciduous forest

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