Question 6 of 25 Submit Consider the reaction: N2 (g) + 3 Br2 (g) =2 NBr3 (g) At equilibrium, the concentrations of N2 and Brz are 0.34 M and 0.70 M respectively, and the concentration of NBR3 is 0.090 M. What is Kc for this equilibrium? 1 2 3 4 C 7 8 +/- x 10 0 LO

What is the equilibrium-constant expression for the following reaction?N2O4 (g)  <--> 2NO2 (g)

The following reaction is at equilibrium and being monitored by a chemist : 2NOF (9) 2NO (g) + F₂ (g) The Chemist measures these concentrations at equilibrium: [NOF] = 0.56M [NO] = 0.32 M [F₂] = 0.28 M What is the equilibrium constant for this reaction?

At a certain temperature, 0.4611 mol of N, and 1.561 mol of H, are placed in a 5.00 L container. N₂(g) + 3H₂(g)2NH₂(g) At equilibrium, 0.1601 mol of N₂ is present. Calculate the equilibrium constant, Ke. Kc = 23.83 Incorrect

After equilibrium is reached in the reaction of 6.30 g H2 with 150. g I2, analysis shows that the 1.00 L flask contains 64.0 g of HI. How many moles of H2, I2, and HI are present in this equilibrium mixture? What is the Keq for this reaction?

Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N2 and Og (from air). N2 (9) + O2(9) - 2NO(9) The equilibrium constant (K.) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.082 mol N, and 0.026 mol O2 per liter, what is the concentration of NO? Concentration = M

Calculate the equillibrium constant using the balanced chemical equation and the concentration of he substances at equilibrium. Based on the calculated value of K which is favored for the reaction products (fwd) or reactants (rev)? 2NO2 (g)= N2O4 (g)     [NO2]=.0760 M [N2O4]=1.26 M