C3H8 (g) 5O2 (g) -> 3CO2 (g) 4H2O (l) in the reaction represented baove, what is the total number of moles of reactants consumed when 1.00 mole of CO2 (g) is produced

The total number of moles of reactants consumed when 1.00 mole of CO₂ (g) is produced is 2 moles.

Explanation:

You have that the balanced reaction is:

C₃H₈ (g) + 5 O₂ (g) ⇒ 3 CO₂ (g) + 4 H₂O (l)

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reactants and products participate in the reaction:

The rule of three or is a way of solving problems of proportionality between three known values and an unknown value, establishing a relationship of proportionality between all of them.

If the relationship between the magnitudes is direct, that is, when one magnitude increases, so does the other (or when one magnitude decreases, so does the other) , the direct rule of three must be applied. To solve a direct rule of three, the following formula must be followed:

a ⇒ b

c ⇒ x

So

where a, b and c are known values. In this case the rule of three is applied as follows: if by stoichiometry of the reaction 3 moles of CO₂ consume 1 mole of C₃H₈, then 1 mole of CO₂ how many moles of C₃H₈ will it consume?

moles of C₃H₈= 0.33

Applying again a new rule of three: if by stoichiometry of the reaction 3 moles of CO₂ consume 5 moles of O₂, then 1 mole of CO₂ how many moles of O₂ will it consume?

moles of O₂=1.67

The total number of moles of reactants consumed will be the sum of the consumed moles of C₃H₈ and the consumed moles of O₂:

0.33 moles + 1.67 moles=2 moles

The total number of moles of reactants consumed when 1.00 mole of CO₂ (g) is produced is 2 moles.

a

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