Question

Which reactant will be used up first if 78.1g of o2 is reacted with 62.4g of c4h10?

A. c4h10
B. o2
C. co2
D. h2o

Answer 1

Reagent O₂ will be consumed first.

Step-by-step explanation:

The balanced reaction between O₂ and C₄H₁₀ is:

2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

Then, by reaction stoichiometry, the following amounts of reactants and products participate in the reaction:

• C₄H₁₀: 2 moles
• O₂: 13 moles
• CO₂: 8 moles
• H₂O: 10 moles

Being:

• C: 12 g/mole
• H: 1 g/mole
• O: 16 g/mole

The molar mass of the compounds that participate in the reaction is:

• C₄H₁₀: 4*12 g/mole + 10*1 g/mole= 58 g/mole
• O₂: 2*16 g/mole= 32 g/mole
• CO₂: 12 g/mole + 2*16 g/mole= 44 g/mole
• H₂O: 2*1 g/mole + 16 g/mole= 18 g/mole

Then, by reaction stoichiometry, the following mass quantities of reactants and products participate in the reaction:

• C₄H₁₀: 2 moles* 58 g/mole= 116 g
• O₂: 13 moles* 32 g/mole= 416 g
• CO₂: 8 moles* 44 g/mole= 352 g
• H₂O: 10 moles* 18 g/mole= 180 g

If 78.1 g of O₂ react, it is possible to apply the following rule of three: if by stoichiometry 416 g of O₂ react with 116 g of C₄H₁₀, 62.4 g of C₄H₁₀ with how much mass of O₂ do they react?

`mass of O_(2) =(416grams of O_(2)*62.4 grams ofC_(4)H_(10) )/(116 grams of C_(4)H_(10))`

mass of O₂= 223.78 grams

But 21.78 grams of O₂ are not available, 78.1 grams are available. Since you have less mass than you need to react with 62.4 g of C₄H₁₀, reagent O₂ will be consumed first.