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

1 Answer
anor277
Jun 6, 2017

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

Explanation:

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

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

Given 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#.

Pressure is a state function of temperature, amount of gas, and volume, so we must make these extra assumptions to answer the question.

Related questions
See all questions in Stoichiometry
Impact of this question
1682 views around the world
You can reuse this answer
Creative Commons License