Suppose a 250. mL flask is filled with 0.60 mol of NO2 and 0.80 mol of...

 

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Suppose a 250. mL flask is filled with 0.60 mol of NO2 and 0.80 mol of O2. 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 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 O₂. You can leave out the M symbol for molarity. NO₂ NO 02 initial ☐ ☐ change ☐ X equilibrium ☐ X Suppose a 250. mL flask is filled with 0.60 mol of NO2 and 0.80 mol of O2. 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 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 O₂. You can leave out the M symbol for molarity. NO₂ NO 02 initial ☐ ☐ change ☐ X equilibrium ☐ X Suppose a 250. mL flask is filled with 0.60 mol of NO2 and 0.80 mol of O2. 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 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 O₂. You can leave out the M symbol for molarity. NO₂ NO 02 initial ☐ ☐ change ☐ X equilibrium ☐ X

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To solve this problem we first need to write the balanced chemical equation for the reaction 2NOg O2... View the full answer