Using the equation shown below, calculate the equilibrium concentration of N2 given that the equilibrium concentration of H2 is 2.0 M and the equilibrium concentration of NH3 is 0.5 M. For the reaction at this temperature, Kc = 2.
N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Using the equation shown below, calculate the equilibrium concentration of N2 given that the equilibrium concentration...
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)
Using the equilibrium constant expression given below, calculate the equilibrium constant if [N2] = 0.063 M, [H2] = 9.2 × 10−3 M, and [NH3] = 1.8 × 10−4 M. Enter your answer in the provided box. Keq = [NH3]2 [N2][H2]3
For the reaction below, Kc = 0.060 at a certain temperature. N2(g) + 3 H2(g) = 2 NH3(g) A flask contains 1.0 M N2, 1.0 M H2, and 1.0 M NH3. Is this system at equilibrium? If not, will the equilibrium concentration of NH3 be greater than, or less than 1.0 M? Justify your answers.
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...
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 = __
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...
10. Using the equation shown below, calculate the equilibrium concentration of each species in a mixture containing 0.0500 M PCls and 5,00 M PCI K for this reaction is 3.33 x 10' at 487 °C. PCs () PC:(8) + Cl() Suvishortliwabidi a llo 11. At equilibrium, the partial pressures of NO2, NO, and O, were found to be 0.200 atm, 0.00026 atm, and 0.600 atm, respectively, in a 1-liter flask. 2NO, (g) 2NO(g) + O2(g) s obomb (a) Write the...
18) Calculate the pressure of N2 if the equilibrium pressures of H2 = 2.0 atm, and NH3 = 0.5 atm, and Kp = 2.0 N2(g) + 3 H2(g) = 2 NH3(g) A) 0.031 atm (B).016 atm C) 0.062 atm D) 62,5 atm E) 0.40 atm 19) Consider the following reaction: CH4(g) + 2 H2S(g) = CS2(g) + 4 H2(g)
At 450°C, ammonia gas will decompose according to the following equation 2 NHa (g)N2 (g)3 H2 (g) Kc 6.30 at 450.C An unknown quantity of NH3 is placed in a reaction flask (with no N2 or Hz) and is allowed to come to equilibrium at 450.0°C. The equilibrium concentration of H2 is then determined to be 0.111 M. Determine the initial concentration of NH3 placed in the flask. Initial concentration NH3 M Evaluate
Calculate KC in terms of molar concentration for the reaction N2(g) + 3H2(g) 2NH3(g) when the equilibrium concentration moles per liter are: N2 = 0.02, H2 = 0.01, NH3 = 0.10.