Question

2. Holg) can be made the direct reaction of the cand clag) in the presence of light. Assume that 6.0g to and 240g cl are mixed in a 10 flank at 28°C and the flask is sealed. a, Provide the balanced chemical reaction b. Calculate the partial pressures of both gases. c. Calculate the total pressure in the flask d. If the temperature was raised to 40°C Calculate the total pressure in the flank. e. Knowing that the day in exceps, calculate, the total pressume of tol in the flask after the reaction - has gone to completion.

Answer 1

(a)

H₂(g)  + Cl₂ (g) $\rightarrow$ 2 HCl(g)

(b)

Number of moles of H₂ = 6.0g/2g/mol = 3 mol

Number of moles of Cl₂ = 240g/70.906g/mol = 3.3848mol

Partial pressure of H₂ = 3mol×0.0821atm.L/K.mol × 301.15K/10L = 7.417atm

Partial pressure of Cl₂ = 3.3848mol×0.0821atm-L/K.mol × 301.15K/10L = 8.3686atm

(c)

Total pressure in the flask = P_H2 + P_Cl2 = 7.417 + 8.3686 = 15.786atm

(d)

Total pressure = n.R.T/V = 6.3848mol × 0.0821× 313.15/ 10 = 16.415atm

= 16.42 atm

(e)

Number of moles of HCl formed = 2 × number of moles H₂ = 3×2 = 6mol

Pressure due to HCl = 6 × 0.0821 × 313.15 / 10 = 15.43atm

Or

If temperature is maintained at 28℃ , then pressure due to HCl = 6 × 0.0821×301.15/10 = 14.83 atm