What mass of O2 is required to produce 14.5 g of CO2 if the reaction has a 65.0 % yield?
CH4 + O2 ® CO2 + H2O

Question

What mass of O2 is required to produce 14.5 g of CO2 if the reaction has a 65.0 % yield?
                          CH4 +  O2 ® CO2 +  H2O

joannablackwelder · Answer

I would use the percent yield and amount of CO2 formed to calculate the theoretical amount of CO2 possible. From this, I can convert to mass of O2 using molar masses and molar ratio.

jfraser · Answer

working backwards, i would start with the 14.5g of $CO_2$ being 65% of the predicted yield, so I'd find the theoretical yield first, then find the mass of $O_2$ that should produce that much $CO_2$

jfraser · Answer

$$65\% yield = \frac{14.5g}{theoretical}$$ and solve for the theoretical mass first