The yeast in rising bread dough converts sugar (sucrose, C12H22O11) into carbon dioxide. A popular recipe for two loaves of French bread requires 1 package of yeast and 1/4 spoon of sugar (about 2.4g) of sugar.
a. Assuming all the carbon in sugar is converted to CO2 gas (i.e. C12H22O11 (s) -> 12 CO2 (g)), what volume of CO2 would be produced at 25 degrees Celsius and 1.03 atm?
b. What would be the volume of CO2 gas produced in part A if the experiment was performed under STP conditions??
Thank you so much!!!!
a. Assuming all the carbon in sugar is converted to CO2 gas (i.e. C12H22O11 (s) -> 12 CO2 (g)), what volume of CO2 would be produced at 25 degrees Celsius and 1.03 atm?
b. What would be the volume of CO2 gas produced in part A if the experiment was performed under STP conditions??
Thank you so much!!!!
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a. First, find the moles of sugar in 2.4g of sugar, then multiply it by 12 because of the molar ratio in the chemical reaction equation. Next, use the Ideal Gas Law PV=nRT
(1.03)(V)=(0.84)(0.08206)(25+273)
V = 19.94 L
b. (1.0)(V)=(0.84)(0.08206)(298)
V = 20.54 L
EDIT -- Whoops, change the 0.84 to 1, since it's 1 mole at STP --> and volume = 22.4 L
(1.03)(V)=(0.84)(0.08206)(25+273)
V = 19.94 L
b. (1.0)(V)=(0.84)(0.08206)(298)
V = 20.54 L
EDIT -- Whoops, change the 0.84 to 1, since it's 1 mole at STP --> and volume = 22.4 L
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Use PV = nRT and you are solving for V, the volume. You have the temperature, although you need to convert it to Kelvin. You also have pressure.
So where do you get n? For every mole of sugar, you get 12 moles of CO2. So how many moles are 2.4 grams of sugar. (actually mmoles of sugar)
At STP, it becomes trivial since one mole of CO2 at STP would occupy 22.4 Liters.
So where do you get n? For every mole of sugar, you get 12 moles of CO2. So how many moles are 2.4 grams of sugar. (actually mmoles of sugar)
At STP, it becomes trivial since one mole of CO2 at STP would occupy 22.4 Liters.
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