Suppose a 500. mL flask is filled with 1.7 mol of N₂ and 0.10 mol of NH3. This reaction becomes possible: N₂(g) + 3H₂(g)2NH₂ (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 N₂. You can leave out the M symbol for molarity. initial change equilibrium N₂ 0 X 0 0 0 NH₂ 0 0 00 X

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?

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

"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 75 L tank with 22. mol of carbon monoxide gas and 26. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 13.5 mol of carbon monoxide gas, 17.5 mol of water vapor and 8.5 mol of hydrogen gas. The engineer then adds another 7.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. || mol x10

Suppose a 250. mL flask is filled with 0.20 mol of N2 and 2.0 mol of NO. The following reaction becomes possible: N2(g) + O2(g) = 2NO(g) The equilibrium constant K for this reaction is 0.693 at the temperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to two decimal places. Шм

Suppose a 250. mL flask is filled with 0.60 mol of N, and 0.70 mol of NO. This reaction becomes possible: N2(g) +0,(g) = 2NO(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. N, NO initial change equilibrium 미미

Suppose a 250. mL flask is filled with 0.30 mol of O, and 1.5 mol of NO. This reaction becomes possible: N, (g) +0,(g) = 2NO(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. alo Ar N2 O2 NO initial change equilibrium

Suppose a 250. mL flask is filled with 1.9 mol of O, and 1.5 mol of NO. The following reaction becomes possible: N2 (g) +0,(g) =2NO(g) The equilibrium constant K for this reaction is 8.51 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. OM

For the reaction 2 NO2 (g) <=> N2O4 (g),  K= 0.67. If [NO2] = 2.0 M, and the [N2O4] = 1.0 M  , which of the following is true?     The reaction is at equilibrium     The reaction will move to the reactant side     The reaction cannot reach equilibrium     The reaction will move to the product side

Suppose a 250. mL flask is filled with 0.90 mol of H, and 0.40 mol of NH,. This reaction becomes possible: 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. N, H, NH, initial ? change equilibrium