Iron(III) oxide and hydrogen react to form iron and water, like this: Fe₂O₂ (s) + 3H₂(g) →2 Fe(s) + 3 H₂O(g) At a certain temperature, a chemist finds that a 3.6 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium ha following composition: compound amount Fe₂O3 3.38 g H₂ Fe H₂O Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. 4.06 g 3.83 g 2.15 g

Suppose a 500. mL flask is filled with 1.0 mol of CO, 1.8 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.932 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐M X 5

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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 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.

Methanol and oxygen react to form carbon dioxide and water, like this: 2 CH,OH(I)+30,(g)-2 Co,(g)+4H,0(g) At a certain temperature, a chemist finds that a 6.3 L reaction vessel containing a mixture of methanol, oxygen, carbon dioxide, and water at equilibrium has the following composition: olo Ar compound amount CH;OH 2.06 g O2 2.63 g CO2 3.06 g H,O 4.20 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0

Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 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. olo Ar N2 H, NH, initial change equilibrium 미

Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant K for this reaction is 1.98 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

"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 50 L tank with 3.5 mol of carbon monoxide gas and 14. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 1.4 mol of carbon monoxide gas, 11.9 mol of water vapor and 2.1 mol of hydrogen gas. The engineer then adds another 0.90 mol of carbon monoxide, 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

For the chemical equation SO₂(g) + NO₂(g) — SO₂(g) + NO(g) the equilibrium constant at a certain temperature is 2.80. At this temperature, calculate the number of moles of NO₂(g) that must be added to 2.20 mol SO₂(g) in order to form 1.00 mol SO3(g) at equilibrium. mol moles of NO₂ (g):