Suppose a 250. mL flask is filled with 1.5 mol of NO₂ and 1.4 mol of NO. This reaction becomes possible: 2NO₂(g) → 2NO(g) + O₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and th equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. initial change NO₂ 0 0 NO 0 0₂ X 00 X

Suppose a 500. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO2. The following reaction becomes possible: NO3(g) + NO(g) - 2NO2(g) The equilibrium constant K for this reaction is 4.37 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 2.0 mol of Cl₂ and 1.2 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl (g) The equilibrium constant K for this reaction is 3.70 at the temperature of the flask. Calculate the equilibrium molarity of C12. Round your answer to two decimal places. Шм 000 Ar

Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N2 and H2 is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H2, 8.0 M N2, and 4.0 M NH3 are present. Determine the initial concentrations of H2 and N2 that were present in the vessel. = N2(g) +3 H2(g) 2 NH3(g) 1 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) N2(g) + 3 H2(g) 2 NH3(g) RESET 0 5.0 8.0 4.0 -4.0 10.0 11.0 -2.0 2.0 -5.0 6.0 -6.0 MAR 22 F2 80 F3 F4 1775 % F5 ག|: MacBook Air 6 < 1 F6 27 & tvill AQ বর F7 E R T Y U Ꮴ $ 54 #3 43 S D F G H DII N&S F8 DD F9 D F10 I' 8 * ∞ ) ) 9 0 0 P J K L

Suppose a 250. mL flask is filled with 0.90 mol of N, and 1.2 mol of NH2. This reaction becomes possible: ME N,(g) +3H,(g) – 2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. H, NH, initial change equilibrium Continue Submit As O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center 43,203 FEB 19 CH.9 PE ASSESS MacBook Air D00 FI0 吕口 F3 F9 esc F5 F7 F2 ロ口 X

Suppose a 250. mL flask is filled with 0.80 mol of O2 and 0.30 mol of SO3. This reaction becomes possible: 2SO2(g) + O2(g) ~ 2SO3(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use r to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity.

Suppose a 500. mL flask is filled with 1.9 mol of N, and 0.20 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 3.27 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places.

Suppose that the equilibrium constant for the chemical reaction   has an equilibrium constant of 2.3 x 107.  What is the equilibrium constant for the reverse reaction?

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 100 L tank with 13. mol of carbon monoxide gas and 23. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 4.0 mol of carbon monoxide gas, 14. mol of water vapor and 9.0 mol of carbon dioxide. The engineer then adds another 8.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 × Ś

reaction K Br(aq) + AgNO3(aq) → KNO3(aq) + AgBr(s) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) 2NaClO₂ (s) 2NaCl (s) + 30₂ (g) 2 HBr(aq) + NaOH(aq) → NaBr(aq) + H,O (1) 00000000000000 type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition X 000 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base Ś