Question

Hydrogen chloride and oxygen react to form chlorine and water, like this:

Answer 1

Answer:

The equilibrium constant Kp for this reaction is 0.0030

Explanation:

Step 1: Data given

Partial pressure at the equilibrium:

pHCl = 76.9 atm

pO2 = 66.3 atm

pCl2 = 40.7 atm

pH2O = 65.1 atm

Step 2: The balanced equation

4 HCl(g) + O2(g) → 2 Cl2(g) + 2 H2O(g)

Step 3: Calculate the equilibrium constant Kp

Kp = ((pH2O²)*(pCl2²)) /(pO2)*(pHCl^4))

Kp =  (65.1²*40.7²) / (66.3*(76.9^4))

Kp = 0.0030

The equilibrium constant Kp for this reaction is 0.0030

Answer 2

Answer:

Kp is 3.03 x 10⁻³ to two significant digits

Explanation:

Kp is the ratio of partial pressure of gaseous produce raised to power of their stiochiometric to the partial pressure of gaseous reactant raised to power of their stiochiometric.

For a reaction: aA + bB ==> cC + dD

$Kp = \frac{|P|C^c * |P|D^d}{|P|A^a * |P|B^b}$

Relating the expression with the given expression and data

A = HCl 76.9 atm    with a = 4

B = O₂ 66.3 atm      with b = 1

C = Cl₂ 40.7 atm      with c = 2

D = H₂O 65.1 atm    with d = 2

$Kp = \frac{40.7^{2}*65.1^{2}}{76.9^{4}*66.3^{1}}$

$Kp = \frac{1,656.49 * 4,238.01}{34,970,783.2321 * 66.3}$

$Kp = \frac{7,020,221.1849}{2,318,562,928.28823}$

Kp = 0.0030278

Kp = 3.0278 x 10⁻³

Kp is 3.03 x 10⁻³ to two significant digits