I have the chemistry equation.
CH4+2O2 -> CO2 +2H2O
how many grams of CO2 are produced from 125g of O2 and excess CH4? I got 172g and says is wrong
CH4+2O2 -> CO2 +2H2O?
- Posted:
- 3+ months ago by mackievicz
- Topics:
- chemistry, equations
Details:
Added 3+ months ago:
solved after hours coming back to it. the 125g of O2 only half is used for CO2 the other Half for H20 then the result matches.
Responses (2)
From the equation, 2 moles of O2 react to produce 1 mole of CO2. Hence ratio O2:CO2 = 2:1. The no. of moles of CO2 produced = 1/2 the no. of moles of O2 reacting.
no. of moles of 02 in 125g,
n(O2) = Mass/Mr(O2)
= 125/32
no. of moles CO2 produced,
n(CO2) = 1/2 * 125/32
= 125/64
mass of CO2 produced
= n(CO2) * Mr(CO2)
= 125/64 * 44
= 85.9375
= 85.9 (to 3 s.f)
The coefficients in the balanced equation determine the ratio of moles of reactants to moles of products. For this reaction, one moles of CH4 reacts with two O2 to produce one mole of CO2 and two moles of H2O. The ratio of O2 to CO2 is 2:1. This means the number moles of CO2 is one half of the number of moles of O2. To determine the number of moles, divide the mass by the mass of one. For O2, the mass of one mole is 32 grams.
Number of moles = 125 ÷ 32 = 3.90625
For CO2, number of moles = ½ * 3.90625 = 1.953125
CO2 = 12 + 32 = 44 grams
This is mass of one mole of carbon dioxide.
Mass of CO2 = 44 * 1.953125 = 85.9375 grams
This is approximately one half of your answer. I hope this is helpful for you. You can round as your instructor desires.