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**gas laws problem (need quick help plz)**

## Homework Statement

ill try to describe the situation as best i can

at first we have a flask (150 ml) with 0.1g of NaHCO

_{3}we attach a syringe with 20ml of acetic acid (CH

_{3}COOH ) to it (and seal it off so nothing escapes)

we inject the acetic acid into the flask and pull the syringe back (so the overall volume doesnt change) the 2 compounds react and produce CO2

the initial(before adding the acetic acid) temp. = 295.6k

initial pressure = 1.020 atm

final temp. = 297.6 k

final pressure = 1.176

what is the initial amount of gas in the flask(in mol)?

and what is the amount of co2 added(in mols)?

what is the partial pressure of CO2

## Homework Equations

ideal gas law equations

## The Attempt at a Solution

i used pv=nrt to calculate the initial amount of gas (using the initial conditions) = 6.45*10

^{-3}mol

for the second part i use PV/nT(initial)=PV/nT(final) to get the amount of mols after the reaction but i get a value less than the first one. this doesnt make sense since we are adding gas to it (note that this was a real experiment and the values might be off from an ideal situation)

can someone help me out with this and maybe hint at what to do on the last 2 parts ?

i really appreciate the help