an air bag was determined to have a maximum volume of 4.5 liters. if the most ef

Question

an air bag was determined to have a maximum volume of 4.5 liters. if the most effective inflation percentage was 95% of the maximum, how much of each reactant below is needed at STP? Acetic acid: 0.250 molar.
NaHCO3(s) + CH3COOH(aq) ---> an air bag was determined to have a maximum volume of 4.5 liters. if the most effective inflation percentage was 95% of the maximum, how much of each reactant below is needed at STP? Acetic acid: 0.250 molar.
NaHCO3(s) + CH3COOH(aq) ---> an air bag was determined to have a maximum volume of 4.5 liters. if the most effective inflation percentage was 95% of the maximum, how much of each reactant below is needed at STP? Acetic acid: 0.250 molar.
NaHCO3(s) + CH3COOH(aq) --->

Explanation / Answer

Solution :-

Balanced reaction equation is as follows

NaHCO3(s) + CH3COOH(aq) ------------ > NaCH3CO2(aq) + H2O(l) + CO2(g)

maximum volume = 4.5 L

and effective inflation percent is 95 %

therefore 4.5 L * 95 % /100 % = 4.275 L

now lets calculate the moles of CO2 at STP in 4.275 L

at STP 1 mol = 22.4 L

therefore

4.275 L * 1 mol / 22.4 L = 0.1908 mol CO2

now lets find the amount of each reactant needed

mole ratio of the CO2 to acetic acid and NaHCO3 is 1 : 1

therefore moles of the CH3COOH needed = 0.1908 mol

moles of NaHCO3 needed = 0.1908 mol

since acetic acid is 0.250 molar

therefore volume of acetic acid needed is

volume of CH3COOH = 0.1908 mol / 0.250 mol per L = 0.763 L

mass of NaHCO3 needed = moles * molar mass

                                        = 0.1908 mol * 84.007 g per mol

                                        = 16.0 g NaHCO3

There we need 0.763 L of 0.250 molar acetic acid (CH3COOH)

and 16.0 g of NaHCO3

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