3NO2(g) K=1.0 × 10-11 N₂O5(g) + NO(g) If a 4.00 L container initially holds 0.13 mol of NO2, how many moles of N₂O5 will be present when this system reaches equilibrium? Enter your answer in scientific notation. moles of N₂O5 - i x 10 i mol

Suppose a 500. mL flask is filled with 0.20 mol of N2 and 1.6 mol of NO. The following reaction becomes possil N2(g) + O2(g) 2NO(g) The equilibrium constant K for this reaction is 0.205 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Шм ✗

Consider the reaction;  N2(g) + O2(g)⇆ 2 NO(g)  where K = 0.10.      Starting with initial concentrations of [N2] = 0.04 M and [O2] = 0.40 M,      the equilibrium concentration of NO is

Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N2(g) + 3H2(g) = 2NH3(g) Ton: N. x10-2 ent (O Pncca waythe chemical system would 5 the vara BI U = E T O Word(s) ------ T T; O Word(s) 5. If the concentration of the product NH3 was increased from 1.0x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B I U E T O Word(s)

For the equilibrium 3NO₂(g) K₂=1.0 x 10-11 N₂O5(g) + NO(g) If a 4.00 L container initially holds 0.25 mol of NO₂, how many moles of N₂O5 will be present when this system reaches equilibrium? Enter your answer in scientific notation. moles of N₂O5 = i x 10 Mi mol

Consider the following reaction. 2 NO₂(g) = N₂O4(g) 4 When the system is at equilibrium, it contains NO₂ at a pressure of 0.860 atm, and N₂O at a pressure of 0.0740 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? atm PNO₂ = atm PN₂0₁ =

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?

A mixture in a 3.67 L flask initially contains 0.763 g H2 and 96.9 g 12. At equilibrium, there is 90.4 g HI. Find Kc for this reaction. H2(g) +12(g) = 2HI(g)

Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 100L tank with 27. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 9.0 mol of nitrogen dioxide gas. The engineer then adds another 6.8 mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol