Question

Be sure to answer all parts.

A) Nitrogen dioxide decomposes according to the reaction
2 NO₂(g) ⇌ 2 NO(g) + O₂(g) where K_p = 4.48 × 10⁻¹³ at a certain temperature. If 0.85 atm of NO₂ is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O₂(g)?
  ___atm O₂
___atm NO

B) For the following reaction, K_p = 0.262 at 1000°C:

C(s) + 2H₂(g) ⇌ CH₄(g)

At equilibrium, the partial pressure of H₂ is 1.20 atm. What is the equilibrium partial pressure of CH₄(g)?

P_CH4(g) = __atm

Answer 1

NO2 0.85 atm Given that 2 (A) Initial Partial pressure of gas= The value of kp for rx n = 4:48 x 10-13 So Chemical Rh quen 2NO, T2NO+O₂ Initial as P. At eam 22 a P-2x 4a3 = 4.48 X 1013 Kp= [22][u 1p-2x3² [0.85-2u on solung the x, we e get = 4.32 x 10-5 atm Partial pressure of the Oxygen gas (Po)= x 4032 x 16 5 atm Partial pressure of No gas Ť (NO) = 20 & 64 x 10 atm ((B) Gruen chemical equation as (cs) + 2H₂(g) F CH4 (9) Gylen that, KP=0.262 at 1000 ° C 6 Peam= 6.20 atm Let the partial partial pressure of the at Pany = P ( let say) egmů

0.262 Kp= Pertu [PH₂]2 P (1•20)2 P= 0.262 x (1-2012 P = 0.3772 atm So Partial pressure of CHu st eam is 0.3772 atm.