First write the equation of the reaction:
reactants: NaHCO3+CH3COOH
products: CH3COONa+CO2+H2O
From the molar masses of
NaHCO3 = 23+1+12+3*16 = 84
CO2 = 12+2*16 = 44
We find the stoichiometric ratio of the two compounds to be
84:44 (approximately)
Hence by proportions/ratios, we find the number of grams, and moles of CO2 produced.
Yes, you need to convert the volume to 22° C and 1.10 atm using PV=nRT, with temperatures being in °K.
Part B is essentially the same as part A, but backwards.
How do you do this? please help. Thank you.
A.) Suppose 2.5 grams of sodium hydrogen carbonate reacts with acetic acid, calculate how many liters of carbon dioxide gas will be produced at 22 degrees celcius and 1.10 atm.
B.) Suppose 0.990 liters of carbon dioxide at 25 degrees celcius and 755 mmHg is produced when sodium hydrogen carbonate reacts with acetic acid. Calculate how many grams of sodium hydrogen carbonate were used to start this reaction.
Also, would you have to use PV=nRT.
for A.) n and v was missing so how do I manipulate it to find both. Is there another equation perhaps? for part B too.
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