At a temperature of 500 K, the equilibrium constant of the reaction 2 NO(g) + O_

Question

At a temperature of 500 K, the equilibrium constant of the reaction 2 NO(g) + O_2(g) 2 NO_2(g) is K_c = 6.9 10^5. At this temperature, a vessel containing a mixture of these gases is found to contain concentrations of 0.012 M NO. 0.20 M O_2, and 0.16 M NO_2. It can be concluded that from this point on the reaction will: The exothermic reaction Si(s) + 2 Cl_2(g) SiCl_4(g) is used in the photovoltaic cell Industry. A mixture of 2 moles of silicon, 0.5 moles of chlorine and 0.1 mole of silicon tetrachloride is placed in a 10-L cylinder equipped with a movable piston at a temperature of 820 degree If 0.2 mole of chlorine is removed from the reaction vessel, the equilibrium will:

Explanation / Answer

Calculate Q

Q = [NO2]^2 / ([NO]^2[O2])

Q = (0.16^2)/((0.012^2)*(0.20)) = 888.8888

If Q < K; then it favours the reactants

7

[Si] = 1 since is solid

[Cl2] ) 0.5/10 = 0.05

[SiCl4] = 0.1/10 = 0.01

Q = [SiCl4]/[Cl2]^2

Q = 0.01 / (0.05^2) = 4

question, if you remove Cl2, then you remove reactants, therefore, the shift goes toward reactants in order to replace the decrease

Shift goes to left

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.