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Liquid methanol (CH3OH) is burned in air to form carbon dioxide and water.?

Author : Mark

Submitted : 2017-11-07 18:07:43    Popularity:     

Tags: CH3OH  burned  Liquid  methanol  air  

How many grams of CO2 are collected at 30C and 1.13 atm if 5.71 mL of
methanol reacted with 1.20 L O2?
ive written out the balanced equation but dont know where to go from here

Answers:

I agree. The question is poorly worded. For the methanol, you need the density to convert to grams to convert to moles. For the O₂, you need realize that temperature and pressure given for the product also apply to the reactant. Use those data to convert to moles. Once you have moles of the two reactants, you have to solve for moles of CO₂ produced to see which is the limiting reactant. Finally you convert to grams of CO₂.

Like any other stoichiometric problem, you need to work in moles.

density = mass / volume

You know the volume of methanol, look up the density and calculate mass. from there, you get moles of methanol.

Use the ideal gas equation to find how many moles of O2 you have.

This is a limiting reactant problem, which one, methanol or O2 runs out first?

the balanced equation with the limiting reactant gives you moles of CO2. mass of CO2 = moles * molar mass of CO2. The P and T doesn't affect the mass of CO2 in this problem.

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