Consider the equilibrium N2(g)+O2(g)+Br2(g)⇌2NOBr(g) Part A Calculate the equilibrium constant Kp for this reaction, given the...

Consider the equilibrium N2(g)+O2(g)+Br2(g)⇌2NOBr(g) Part A Calculate the equilibrium constant Kp for this reaction, given the following information (at 295 K ): 2NO(g)+Br2(g)⇌2NOBr(g)Kc=2.1 2NO(g)⇌N2(g)+O2(g)Kc=2.2×1030 Express your answer using two significant figures.

Expert Solution

queen_honey_blossom answered 2 years ago

The equilibrium constant, Kp, for the followingreaction is 0.160 at 298K.2NOBr(g) 2NO(g)+ Br2(g)...

The equilibrium constant, Kp, for the following reaction is 0.160 at 298K.2NOBr(g) → 2NO(g) + Br2(g)If an equilibrium mixture of the three gases in a 17.3 L container at 298K contains NOBr at a pressure of 0.351 atm and NO at a pressure of 0.222 atm, the equilibrium partial pressure of Br2 is atm.

The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g)<====> 2NO(g) + Br2(g)...

The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g)<====> 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 16.4 L container at 298K contains 0.383 mol of NOBr(g) and 0.230 mol of NO, the equilibrium concentration of Br2 is____M The equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K. NH4I(s) <====>NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 5.04 L container at 673...

Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K...

Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K = 1.7 × 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species. to the right to the left [N2] =____ mol/L [O2] = ____mol/L [NO]...

The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =...

The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP = 0.032 at a particular temperature. At that temperature, a vessel is filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm of NO (g). What is the pressure of NO (g) at equilibrium?

Consider the following equilibrium: 2NOBr(g) <------> 2NO(g) + Br2(g). An equilibrium mixture is 0.146 M NOBr,...

Consider the following equilibrium: 2NOBr(g) <------> 2NO(g) + Br2(g). An equilibrium mixture is 0.146 M NOBr, 0.270 M NO, and 0.236 M Br2. a) What is the value of Kc at the temperature of the above concentrations? b) How many moles/liter of NOBr must be added to the above equilibrium mixture to produce an equilibrium mixture that is 0.439 M Br2? c) If the temperature is 370 K, what is the value of Kp? d) What is the value of...

At 850K, the value of the equilibrium constant Kp for the ammonia synthesis reaction: N2(g)+H2(g)--> N2H2(g)...

At 850K, the value of the equilibrium constant Kp for the ammonia synthesis reaction: N2(g)+H2(g)--> N2H2(g) is 0.3290. If a vessel contains an initial reaction mixture in which [N2]= 0.0200 M, [H2]=0.0200 M, and [N2H2]= 0.000150 M, what will the [N2H2] be when equilibrium is reached? The answer is not: 0.000298, .00681, .000172, .000148, .00031, .00471 please help!

Consider the following equilibrium: 2NOBr(g) 2NO(g) + Br2(g) An equilibrium mixture is 0.150 M NOBr, 0.395...

Consider the following equilibrium: 2NOBr(g) 2NO(g) + Br2(g) An equilibrium mixture is 0.150 M NOBr, 0.395 M NO, and 0.221 M Br2. a) What is the value of Kc at the temperature of the above concentrations? Kc = M b) How many moles/liter of NOBr must be added to the above equilibrium mixture to produce an equilibrium mixture that is 0.448 M Br2? mol/L NOBr must be added c) If the temperature is 400 K, what is the value of...

PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2...

PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2 4.K=2[NO][N2][O2] PART B. The equilibrium-constant of the reaction NO2(g)+NO3(g)⇌N2O5(g) is K=2.1×10−20. What can be said about this reaction? 1.At equilibrium the concentration of products and reactants is about the same. 2.At equilibrium the concentration of products is much greater than the concentration of reactants. 3.At equilibrium the concentration of reactants is much greater than that of products. 4.There are no reactants left over once...

At a particular temperature Kp = 0.041 for the reaction N2(g) + O2(g) ⇄ 2NO(g) What...

At a particular temperature Kp = 0.041 for the reaction N2(g) + O2(g) ⇄ 2NO(g) What is the equilibrium partial pressure of NO if a flask initially contains 0.12 atm of all three gases? Report the pressure of NO in atm rounded to the nearest hundredth of an atm.

At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4×103. The initial concentration of...

At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4×103. The initial concentration of NO is 0.250 M . Part A What is the equilibrium concentration of NO? Part B What is the equilibrium concentration of N2? Part C What is the equilibrium concentration of O2? Please show me how to got your results :) Thank you!

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