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

Reagent O₂ will be consumed first.

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 molesO₂: 13 moles CO₂: 8 moles H₂O: 10 moles

Being:

C: 12 g/moleH: 1 g/moleO: 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/moleO₂: 2*16 g/mole= 32 g/moleCO₂: 12 g/mole + 2*16 g/mole= 44 g/moleH₂O: 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 gO₂: 13 moles* 32 g/mole= 416 gCO₂: 8 moles* 44 g/mole= 352 gH₂O: 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 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.

The gas would begin to expand, and eventually the can would burst or explode.

Mass of water is smething that you froma drug test or sum girl ya