Suppose a 500. mL flask is filled with 0.50 mol of N, and 0.90 mol of NO. This reaction becomes possible: N,(g) + O,(g) – 2 NO(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. NO initial 1.0 ? change -2x +x equilibrium 1+x 1.0 - 2x

Suppose a 500. mL flask is filled with 1.6 mol of N₂ and 0.40 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) 2NO(g) The equilibrium constant K for this reaction is 6.10 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. M X Ś

Suppose à 250. mL flask is filled with 1.3 mol of CO, 1.8 mol of H,O and 1.6 mol of H,. This reaction becomes possible: co() +H,0(g) =CO,e)+H,(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 H,. You can leave out the M symbol for molarity. CO H,0 Co, H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Roserved Terms of Use Privacy 1 Ace O Type here to search

I am confused because I am getting two possible answers one being 10. 6 and the other being 1.38

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 125 L tank with 47. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 22. mol of nitrogen dioxide gas. The engineer then adds another 16. 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 x10

Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.80 mol of NO and 0.70 mol of CO,. The following reaction becomes possible: 2' NO, (g) +CO(g) - NO(g)+CO,(g) The equilibrium constant K for this reaction is 6.92 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. olo Ar OM ?

"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 125 L tank with 20. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.0 mol of carbon monoxide gas, 11. mol of water vapor and 13. mol of carbon dioxide. The engineer then adds another 7.0 mol of carbon monoxide, 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

"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 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 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

Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 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 O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium

Write the equilibrium 6H2O(g) + 6CO2(g) C6H12O6(s) + 6O2(g)