The reaction 2 NO+Cl2 2 NOCl is at equilibrium at 25'C when PNo-0.24 atm, Pc 0.61...
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
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
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
Consider the following equilibrium: Now suppose a reaction vessel is filled with 2.96 atm of nitrogen monoxide (NO) and 5.86 atm of nitrosyl chloride (NOCI) at 1137. °C. Answer the following questions about this system rise x10 Under these conditions, will the pressure of NOCl tend to rise or fall? fall Is it possible to reverse this tendency by adding C12? In other words, if you said the pressure of NOCl will tend to rise, can that be changed to...
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
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)
The equilibrium constant Kp for the reaction PCl5(g) <---> PCl3(g) + Cl2(g) is 1.15 at 25 degrees Celsius. The reaction starts with a mixture of 0.177 atm PCl5, 0.223 atm PCl3, and 0.111 atm Cl2. When this mixture comes to equilibrium at 25 degrees Celsius, what are the equilibrium pressures of each component?
0.0950 atm, PC120.171 atm, and PNOCI QUESTION 14 What is the equilibrium constant, Kp. for the reaction below if the equilibrium partial pressures are PNO 0.280 atm? 2 NO(g) + Cl2 (8) 2 NOCI (g) 4. 4.55 x 10-3 5.5.80 x 10-2 17.2 d. 50.8 e 1.97 x 10-2
Consider the following reaction: 2 NO(g) + Cl2(g) = 2 NOCI() The reaction is at equilibrium at 125 °C with PNo = 1.66 bar, PcI2 = 0.830 bar, and PNoci = 1.09 bar. (a) Calculate the value of the equilibrium constant of this reaction at 125 °C. (b) Calculate the value of AGº of this reaction at 125 °C. Give you answer with 3 significant figures and in the units kJ/mol. (c) Given the following additional information and assuming that...
23. Consider the reaction: 2 NO (g) C12 (g)-2 NOCI (g) + Suppose a mixture at equilibrium (under standard conditions at 350 K) contains the gases at the following pressures: NO: 0.150 atm Cl2: 0.071 atm NOCI: 14.6 atm Calculate Keq and then use this value to calculate ΔGo at 350 K. 0Jd. -29.2 k e. -14.9 k a. +34.3 kJ b. -34.3 kJ c. -21.0