Question

According to the equation below, how many liters of hydrogen sulfide gas can be produced from 1.50L of 3.00M HCl at 295K and 1.50atm? Al 2 S 3 (aq) + 6 HCl(aq) ---> 2 AlCl 3 (aq) + 3 H 2 S(g)

I was able to find a similar problem but I am not understanding the steps. If someone could please do step by step I'd appreciate it. Also I believe the formula is PV=nrt but since it already gives you a volume I am confused.

Thank you

Answer 1

note:- just you have to find the moles of H2S then calculate the volume from it

the reaction is

Al 2 S 3 (aq) + 6 HCl(aq) ---> 2 AlCl 3 (aq) + 3 H 2 S(g)

Since we know that

no of moles = molarity * volume in L = 3.00*1.5 = 4.5 moles of HCl

1 mol of HCl produces 0.5 mol of H2S

so

4.5 mol of HCl will produce 2.25 mol of H2S

now we know that

V = nRT/P

n = 2.25 mol

R = 0.082057 Latm/mol-K

T = 295K

P =  1.50atm

V = 2.25*0.082057*295 / 1.50

V = 36.3 L Answer

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