At high temperature, HCl and O2 react as 4HCl(g) O2(g) 2Cl2(g) 2H2O(g) If HCl at 2. 30 atm and O2(g) at 1. 00 atm react at 75 0 K, the equilibrium pressure of Cl2(g) is 0. 93 atm. Calculate K.

Kc = 2300 L·Atm·mol⁻¹

Explanation:

                 4HCl(g)       +           O₂(g)         =>         2Cl₂(g)          +  2H₂O(g)

P(i)              2.3 atm                1.00 atm                    0                                 0

ΔP                 -4x                          -x                       +2x                             +2x

P(eq)           2.3-4x                     1.00-x                    2x                                2x

Given P(Cl₂) at equil. = 0.93 atm => 2x = 0.93 => x = 0.465 atm

P(eq)  [2.3-4(0.465)]atm     1.00-0.465atm           2(0.465)atm      2(0.465)atm

                 = 0.44 atm              = 0.535 atm               = 0.93 atm        =0.93 atm

Kp = (P(Cl₂))²(P(H₂O))²/(P(HCl))⁴(P(O₂))¹ = (0.93)²(0.93)²/(0.44)⁴(0.535)¹ atm⁻¹ = 37.3 atm⁻¹

Kc = Kp(R·T)^-Δn = 37.3(0.08206)(750)⁻⁽⁻¹⁾ L·atm·mol⁻¹ = 2296 L·atm·mol⁻¹ ≅ 2300 L·atm·mol⁻¹

answer; /// the amount of material dissolved in a measure of liquid(concentration) the above statement is (true); /// good luck

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