I need big help with lab homework. Of Course, this volume is only approximate as

Question

I need big help with lab homework.

Of Course, this volume is only approximate as the width of the inflated bag is not uniform. To get a better value for the volume, you fill the bag with water, then measure the volume of the water to be 1274.7mL. Now you measure room temperature to be 21C and the barometer on the wall gives a reading of 756 torr for the atmospheric pressure. Using the ideal gas law, calculate the number of moles of CO2 that will be required to fill the bag at this temperature and pressure.

Now inspect the reactions above generating CO2 and caluclate the molar quanity of NaHCO3 and CH3COOH needed.

Quantity of NaHCO3:

Quantity of CH2COOH:

What mass of NaHCO3 will be needed?

You have a solution of 6.03M acetic acid. What volume of this solution will be needed.

Explanation / Answer

a)

using the gas law PV=nRT and solving for n. Convert C to K, mL to L, and Torr to atm.

1274.7mL = 1.2747L

756 torr = .9947 atm

21C = 294 K

R (gas constant) = .0821

Now you can plug in and find n (PV/RT=n)

(.9947)(1.2747)/(.0821)(294) = 5.25*10^-2 mol

b)

Using the formula Molarity = number of moles / volume (M=n/v) you can calculate the volume needed.

5.25*10^-2 mol/6.03M = n

.0087L or 8.7mL

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