If 6.5 grams of CO react, how many liters of #CO_2# are produce?

Answer 1

You need to specify standard conditions of temperature and pressure, for instance, #1*atm#, and #298*K#.....and get approx. #160*L#

Now carbon monoxide oxidizes to give the same molar quantity of #CO_2#:

#CO(g) + 1/2O_2(g) rarr CO_2(g)#

Considering the Ideal Gas Equation...

#V=(nRT)/P=((6.5*g)/(28.01*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx298*K)/(1*atm)#

#~=160*L#.

We need to make these additional assumptions in order to respond to the question because pressure is a state function of temperature, gas volume, and amount.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer 2

Wyatt Adkins

Use the stoichiometric coefficients from the balanced equation to find the moles of CO reacting. Then, apply the ideal gas law (PV = nRT) using the conditions provided to calculate the volume of CO₂ produced.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.