Iron(III) oxide reacts with carbon monoxide gas to produce iron metal and carbon dioxide gas. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) In this reaction, 3 moles of CO gas is needed to completely react with every 1 mole of iron(III) oxide. You add exactly 1 mole of Fe2O3 to your reaction flask. However, what if you had MORE than 3 moles of CO gas in your reaction flask? What would happen? Would the reaction just keep going, and make more products? Describe what you think would happen, including WHAT SPECIFIC COMPOUNDS would be present in the flask at the end of the entire reaction.

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

if the temperature drops and becomes cool

then the atmosphere can be freezing as the water vapor in the air is at maximum (100%) and can be severely cold

also can be snowing lightly as the moisture in the air will start to solidify

and btw this is not chemistry but