If 10.00 moles of copper are reacted with 6.00 moles of sulfur according to the following balanced equation, which reactant is the limiter and how many moles of excess reactant would remain after the reaction is completed? 2 Cu + S --> Cu2S Cu is limiting and 1.00 mole of excess S remain

S is limiting and 1.00 moles of excess Cu remain

S is limiting and 4.00 moles of excess Cu remain

Cu is limiting and 4.00 moles of excess S remain

Cu is limiting and 1.00 mole of excess S remain

Explanation:

The chemical balanced reaction is:

According to stoichiometry :

2 moles of require 1 mole of

Thus 10.00 moles of will require=  of

Thus is the limiting reagent as it limits the formation of product and is the excess reagent.

Moles of S left = (6.00-5.00) moles = 1.00 mole

Thus Cu is limiting and 1.00 mole of excess S remain.

um i think it might be a car?

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