Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: tinkas22 on May 18, 2009, 06:14:45 PM
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Find the mass of sugar (C6H12O6) required to produce 1.82 L of carbon dioxide gas at STP from the reaction described by the following equation:
The balanced equation is
C6H12O6 :rarrow: 2C2H6O+2CO2
I don't know how to start out the problem.. My chem teacher won't help us...
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Dear tinkas22;
Again: - That’s a normal "Stoichiometry Problem".
Translate the Volume of CO2 generated into moles with the help of the “Molar Volume of Gas” (MVoG) according to the table below:
http://en.wikipedia.org/wiki/Standard_temperature_and_pressure#Molar_volume_of_a_gas
Take care for what STP should mean, there are different meanings of it!
I would suggest for STP: 0°C and 1 atm; then the MVoG will be 22.41 L/mole.
Good Luck!
ARGOS++
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Hellow...i'm gerry from Indonesia, maybe I could help you a little to help your case. the first thing you have to do is convert volume carbon dioxide into mole unit. how? STP means the condition of this reaction is ----> 22.4 liter per mole. thus, now you'll have the mole of CO2. after that, see the completed reaction, mole ratio of glucose is a half of the carbon dioxide one. That means, now you know your glucose's mole. How weight is it? use this general equation: m = n x Mr....well then.....you'll get everything clear.. :)