2 NOCl(g) ⇄ 2 NO(g) + Cl2(g) Kp = 7.2×
10-6
1.50 atm of NOCl(g) is placed in a container and the system is
allowed to reach equilibrium. Calculate the equilibrium pressure of
Cl2(g) at equilibrium.
4.8 × 10-2 atm
8.5 × 10-3 atm
3.2 × 10-2 atm
2.4 × 10-2 atm
1.6 × 10-2 atm
2 NOCl(g) ⇄ 2 NO(g) + Cl2(g) Kp = 7.2× 10-6 1.50 atm of NOCl(g) is...
3. Calculate P [NO]eq, if P [NOCl]eq = 0.60 atm, P [Cl2]eq = 1.50 atm, and Kp = 3.9 × 10-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)
Calculate P [NO]eq, if P [NOCl]eq = 0.33 atm, P [Cl2]eq = 0.50 atm, and Kp = 1.9 x 10-2.2 NOCl(g) ?? 2 NO(g) + Cl2(g)13)A) 1.7 atm B) 0.30 atm C) 0.0042 atm D) 0.087 atm E) 0.064 atm
6) Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with an initial pressure of 10.0 atm comes to equilibrium according to this reaction: 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) KP=4.0×10−4
For the equilibrium 2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 at 150 ∘C. a.)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? b.)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? c.)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of Br2 after equilibrium is reached? a.)If 2.7×10−2 atm of IBr is...
At a particular temperature, Kp-0.39 for the reaction below. N204(g) 2 NO2(g) (a) A flask containing only N204 at an initial pressure of 4.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. N2O4 NO2 atm (b) A flask containing only NO2 at an initial pressure of 9.6 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. No2 (e) From your answers to parts (e) and (b), does it matter...
saw an answer posted already, but think it is wrong as they used
Kp = [NOCL]^2/ [NO]^2 x [Cl2]. In this question, NOCl is the
reactant, and I thought Kp = [products] / [reactants]
An evacuated reaction vessel is filled with 3.60 atm of NOCI. When the system reaches equilibrium according to the reaction below, there are 0.160 atm of NOCI. What is Kp for this reaction? 2 NO (g) + Cl2 (g) = 2 NOCI (g)
Consider the following equilibrium: 2NOCl(g) ⇌ 2 NO(g) + Cl2(g) Kc = 1.6 x 10-5 1.00 mole of pure NOCl and 1.00 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of NO(g)
For the equilibrium 2IBr(g)?I2(g)+Br2(g) Kp=8.5×10?3at 150 ?C. Part A If 2.2×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B If 2.2×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? Express your answer to two significant figures and include the...
The equilibrium constant, Kc, for the reaction 2 NOCl (g) ⇄ 2 NO (g) + Cl2 (g) is 2.4 x 10-7. What is the equilibrium constant for the reaction Cl2 (g) + 2 NO (g) ⇄ 2 NOCl
For the equilibrium 2IBr(g) ⇌ I2:(g) + Br2(g) Kp = 8.5 x 10-3 at 150°C. Part A If 2.9x10-2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached?