Multiple Choice
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) 
2NO(g)
The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?
A) 0.16 atm
B) 0.31 atm
C) 3.1 atm
D) 7.7 atm
E) 7.8 atm
Correct Answer:
Verified
Correct Answer:
Verified
Q14: The two equilibrium constants for the same
Q61: For some gas-phase reactions, K<sub>p</sub> = K<sub>c</sub>.
Q71: The following reaction is at equilibrium at
Q72: Write the mass-action expression, <img src="https://d2lvgg3v3hfg70.cloudfront.net/TB7800/.jpg" alt="Write
Q74: At high temperatures, carbon reacts with O<sub>2</sub>
Q75: Consider the equilibrium reaction: N<sub>2</sub>O<sub>4</sub>(g) <img src="https://d2lvgg3v3hfg70.cloudfront.net/TB7800/.jpg"
Q77: At 450°C, tert-butyl alcohol decomposes into water
Q78: Nitrogen dioxide can dissociate to nitric oxide
Q80: At 500°C the equilibrium constant, K<sub>p</sub>, is
Q81: About half of the sodium carbonate produced