For the reaction N2O4(g)<--->2NO2(g) Kp = 0.148 at a temperature of 298 K. What is Kp for the following reaction? 10NO2(g)<--->5N2O4(g)

The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =

Suppose a flask contains CH4 at a pressure of 1.80 atm. The reaction below then proceeds to equilibrium.  If KP = 0.0152, what are PH2 and PCH4 at equilibrium?  Set up the ICE problem, then solve it.                  CH4 (g)    =    C(s)     +     2 H2 (g)

Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂ (g) S₂Cl₂(g) + CCL (g) Suppose 1.20 mol of CS₂ and 3.60 mol of Cl₂ were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.23 mol CCl4. Calculate Ke at the unknown temperature. Ke- Submit Answer Try Another Version References] 10 item attempts remaining

In a study of the formation of NOx air pollution, a chamber heated to 2200°C was filled with air (0.790 atm N2, 0.210 atm O2). What are the equilibrium partial pressures of N2, O2, and NO if Kp = 0.0460  for the following reaction:N2​(g)+O2​(g) <---> 2NO(g) What is P(N2)? Units are in atm

A flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g) at 25 °C, and the following equilibrium is achieved: N2O4(g) ⇋ 2NO2(g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.1.What is the equilibrium partial pressure of N2O4? 2.Calculate the value of Kp for the reaction.

a) You are working with an equilibrium of the following system:                          2SO2 (g) + O2 (g) <--> 2SO3 (g) If each of the reactants and products has a partial pressure of 0.325 atm at equilibrium, what is the kp?  b) What is the Kc for the reaction above if it takes place at 400oC?