The value of Kp for the reaction below is is 4.30 × 10–4 at 648 K.
3H2(g)+N2(g)----> 2NH3(g)
Part 1) Determine the equilibrium partial pressure of NH3 in a reaction vessel that initially contained 0.900 atm N2 and 0.500 atm H2 at 648 K.
_______atm
The value of Kp for the reaction below is is 4.30 × 10–4 at 648 K....
For the reaction represented below, the value of the equilibrium constant, Kp is 3.1 × 10-4 at 700 K. N2 (g) + 3H2 (g) ⇌ 2NH3 (g) Assume that the initial partial pressures of the gases are as follows: P(N2) = 0.411 atm, P(H2) = 0.903 atm, and P(NH3) = 0.224 atm. Which of the following is true? Q < K Q > K Q = K
The equilibrium constant, Kp, is 4.51 x 10-35 at 450c for the reaction expressed below. N2 (g) + 3H2 (g) equilibrium arrows 2 NH3 (g) a. Write the equilibrium expression for, Kp, for the reaction. b. Supposed you start out with only reactants in a rigid container. The initial partial pressure of N2 (g) is 1 atm and that of H2 is 1.4 atm. What ate the partial pressure of each species when the system reaches equilibrium? Can you explain...
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An evacuated (.e. empty) vessel is charged with 84.9 atm of NH3 (g). The following reaction proceeds to reach equilibrium. 2NH3(g) = N2(g) + 3H2(g) At equilibrium, the partial pressure of H2 remains constant at 64.3 atm. The value of Kp is Report your answer to 3 significant figures. Use scientific notation, i.e. 1.23E4.
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12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) + 3 H2(g) 2 NH3(g) a. Write the equilibrium expression, Kp, for the reaction. b.Suppose y ou start out with only reactants in a rigid container. The initial partial pressure of N2(g) is 1.0 atm and that of H2(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium? c. Find K, for this process at 450°C.
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