3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g)
b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc
c) Calculate the Kp for this reaction
d) Is the equilibrium mixture mostly reactants or products?
e) Does this reaction go to nearly 100% completion? Explain
f) If Qc = 2.5 x 10-3 which direction is the reaction proceeding? Explain
g) If Qc = 2.5 x 105 which direction is the reaction proceeding? Explain
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2...
The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2 NH3(g) Kc=? Write the equilibrium constant expression (Kc) for this reaction. Calculate the value of Kc at 500. K for the formation of ammonia in part a) using the following measured concentrations for the equilibrium mixture: [N2] = 3.0 x 10-‐2 M; [H2] = 3.7 x 10-‐2 M; [NH3] = 1.6 x 10-‐2 M. [1.7 x 102] Now, calculate the value of Kc for the formation of...
A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.61 M, [H2] = 1.26 M, and [NH3] = 0.30 M. Calculate the equilibrium constant, Kc, if the reaction is represented as ( 1 2 ) N2(g) + ( 3 2 ) H2(g) ⇌ NH3(g)
Consider the following reaction at 350oC: N2(g) + 3 H2(g) ⇌ 2 NH3(g); Kc=70. If the concentrations in the reaction mixture at some moment of time are: [NH3] = 0.0100 M, [H2] = 0.0415 M and [N2] = 0.0200M , then Group of answer choices the system is at equilibrium and no net change will occur the system is not at equilibrium and the reaction will proceed to the left the system is at equilibrium and the reaction will proceed to...
For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105. Use the given concentrations to determine the following. [N2] = 0.0028 M [H2] = 0.0045 M [NH3] = 0.30 M (a) Determine Q at this time. (Omit units.)
Please help i need to get these right in order to get an A PLEASE PLEASE PLEASE 1. What is the Kc for the following reaction at equilibrium at 1000 ∘C if [CO]= 0.50 M , [H2]= 0.32 M , [CH4]= 1.6 M , and [H2O]= 2.8 M ? CO(g)+3H2(g)⇌CH4(g)+H2O(g) 2. The equilibrium constant, Kc, for the reaction of H2 and N2 is 1.7×102 at 225 ∘C. 3H2(g)+N2(g)←−→2NH3(g) If the system at equilibrium contains 0.19 M H2 and 0.026 M...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C The value of Kp for this reaction is a. less than ko O b.greater than kc O c equal than ke Consider the reaction: N2 (g)+3 H2 (g)=2 NH3 (g)Kc = 0.0043T = 300 °C Part 1. Given the initial conditions below, which statement is true? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M O a. Q is greater...
an equilibrium mixture is analyzed and found to contain 0.94M N2 , 0.701M H2 and .35 M NH3 at room temp. A. what is Kc for reaction N2(g) +3H2(g) -> 2NH3 (g) ? B. write out the relationship between Kc and Kp, then calc Kp at 25C please show all work
Be sure to answer all parts. A) Calculate Kp for the following equilibrium: 3 O2(g) ⇌ 2 O3(g) Kc =1.8 × 10 −56 at 450 K __× 10__ B) Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0233 M, [N2] = 0.119 M, and [H2] = 0.369 M. Calculate Kc for the reaction at this temperature. Kc = __
For the Equilibrium System N2 (g) + O2 (g) === 2 NO (g) 1.) Write a Kc and a Kp expression. 2.) If Kc = 1.50 x 10-2 at 653oC, Calculate and report the equilibrium concentrations of all of the reactants and all of the products at 653oC, if the initial concentrations were [N2]0 = 0.0100 M [O2]0 = 0.0200 M [NO]0 = 0.00300 M 3.) Calculate Kp for this equilibrium system at 653oC using the equation Kp = Kc(RT)∆n....
The equilibrium constant for the chemical equation N2(g) 3 H2(g)2NH3 (g) is Kp = 0.0146 at 183 oC. Calculate the value of Kc for the reaction at 183 °C.