For the reaction: N_2(g) + O_2(g) 2NO(g) If 0.200 moles of NO gas is placed in...
For the reaction: N_2(g) + O_2(g) = 2 NO(g) K_c = 4.0 at a particular temperature. Suppose we begin an experiment by mixing 0.1 mol of N_2 and 0.1 mol of O_2 in a 1.0-liter container. What will be the concentration of NO (in mol/L) once equilibrium is reached at the given temperature? [enter number with one decimal place]
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction the equilibrium will shift if: N_2 is added? H_2 is removed? NH_3 is added? NH_3 is removed? the volume of the container is decreased? the pressure is increased by adding Argon gas? the reaction is cooled? equal number of moles of H_2 and NH_3 are added? a catalyst is added The equilibrium constant for the following reaction is 5.0 at 400 degree C. CO_(g)...
A mixture of 0.200 moles of N2O and 0.100 moles of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 N2O(g) + O2(g) ↔ 4 NO(g) At equilibrium, 0.196 moles of NO is present. What is the composition of the equilibrium mixture in terms of moles of each substance present? A 0.178 mole sample of C2H6 and a 0.329 moles sample of H2 are placed in a reaction container and allowed to react...
For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container. A(g) + 2B(g) C(g) At equilibrium, the concentration of A is 0.210 mol/L. What is the value of K?
Consider the equilibrium reaction: 2NO(g) + O_2(g) 2NO_2(g) Delta H = +114.6 kJ What will be the change in the equilibrium concentration of NO_2 under each of the following conditions? Considering each change separately, state the effect (increase, I; decrease, D; or no change NC) specified). a) O_2 is added ___ b) energy is added___ c) NO is removed ___ d) a catalyst is added ___ e) it is placed in an ice bath ___ f) the volume is increased...
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
For the reaction A(g)+2B(g)--><--- C9g) 2 moles of A and 3 moles of B are placed in a 6.00 Liter container. At equilibrium, the concentration of A is .300mol/L. What is the concentration of B at equilibrium and what is the value of K?
At some temperature, the Kc for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) is 1.6 x 10^-5. Calculate the concentrations of all species at equilibrium if 1.0 moles of pure NOCl is initially placed in a 2.0 L flask
A mixture of gas consists of 10 g N_2, 10 g O_2, and 10 g C_2H_2. What are the mole fractions of each gas? X_N2 X_O2 X_C2H4 0.357 0.313 0.385 0.333 0.333 0.333 0.326 0.372 0.302 0.339 0.296 0.365 0.357 0.313 0.250
2NO(g) + Br_2(g) A reaction mixture was found to contain 8.57xl0^-2 moles of NOBr(g), 4.62xl0^-2 moles of NO(g), and 3.66xl0^-2 moles of Br2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q_c, equals The reaction must run in the forward direction to reach equilibrium. must run in the reverse direction to reach equilibrium. is at equilibrium.