Industrially, hydrogen chloride gas is made by the combination of hydrogen and c
ID: 535668 • Letter: I
Question
Industrially, hydrogen chloride gas is made by the combination of hydrogen and chlorine, the reaction being quantitative. If a mixture of 362 mL of hydrogen and 345 ml of chlorine is caused to react, H_2(g) + Cl_2(g) rightarrow 2 HCl_(g) a. how many milliliters of H_2 will be present after reaction has taken place? _____ b. how many milliliters of Cl_2 will be present?_____ c. how many milliliters of HCl will be present? _____ [All volumes are made under the same conditions of temperature and pressure.] At the boiling point of liquid nitrogen (-195.8 degree C), the density of liquid nitrogen is 0.8081 g/mL. What is the volume of 1.000 mol of: (a) N_2(l) at -195.8 degree C (b) N_2(g) at 20.0 degree C and 1.000 atm?Explanation / Answer
1) The reaction between H2 and Cl2 is given by
H2 + Cl2 -----> 2HCl
1vol. of H2 reacts with 1vol. of Cl2 to produce 2vol. of HCl
Given that 362mL of H2 and 345mL of Cl2, Cl2 is the limiting reagent and H2 is excess reagent
in 362mL of H2 345mL reacts with Cl2 to form 2*345 ml of HCl
Thus, H2 left after completion of reaction = 362-345 = 17mL
The Cl2 left after completion of reaction = 345-345 = 0.0 mL
The HCl formed after reaction = 2*345 = 790mL
2) Given that, density of N2 at its BP = 0.808 g/mL
(1mole of N2 = 14g, Volume = mass/density)
a) then volume of 1.0 mole of N2 at its BP = 14/0.808 = 17.326 mL
b) volume of N2 at 20 deg, 1.00 atm pressure
we know that, ideal gas equation PV=nRT
V = nRT/P = 1.00mol*0.0821L.atm.K^-1*293 K/1.00 atm = 24.055 mL