Assuming total mass to be 100 g
Mass of C = 52.93 g
=> Moles of C =
Mass of H = 5.92 g
=> Moles of H=
Mass of N = 41.15 g
=>Moles of N=
Simplest mole ratio of the atoms in the compound:
Empirical formula mass=
Multiple n =
Molecular formula=
Answer: 0.887 g of should be added to excess HCl(aq).
Explanation:
According to ideal gas equation:
P = pressure of gas = 805 torr = 1.06 atm (760torr=1atm)
V = Volume of gas = 235 ml = 0.235 L
n = number of moles = ?
R = gas constant =
T =temperature =
According to stoichiometry:
1 mole of chlorine is produced by = 1 mole of
Thus 0.0102 moles of chlorine is produced by = moles of
Mass of =
0.887 g of should be added to excess HCl(aq).
which means that the volume increased by 26.4 mL in order to compensate for the decrease in pressure.
Like I said, depends on what your initial volume was, but that's how you think of it.
Hope this helped!