Song up a reaction Suppose a 500 ml flask is filled with 0.90 mol of CH4,...
Suppose a 500 ml flask is filled with 0.30 mol of CH4, 0.60 mol of H20 and 1.3 mol of CO. This reaction becomes possible: CH (8) + H20(8) -CO(g) + 3H2(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...
Suppose a 500. mL flask is filled with 0.60 mol of CH, 0.70 mol of CO and 0.10 mol of H,. This reaction becomes possible: CH4(8)+H20(g)Co (g)+3H2(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 H2O. You...
Suppose a 250. mL flask is filled with 1.7 mol of H2S, 2.0 mol of CS2 and 0.50 mol of H 2. This reaction becomes possible: CH_(8) +2H2S(g) = CS2(g) + 4H2 () 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...
Suppose a 250 ml flask is filled with 0.20 mol of So, and 1.3 mol of SOz. This reaction becomes possible: 250,() +0,6) - 2503() 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...
Suppose a 500. mL flask is filled with 2.0 mol of SO, and 1.8 mol of O,. This reaction becomes possible: 2SO2(g)+02(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 x to stand for the unknown change in the molarity of O. You can leave out the M...
Suppose a 500 ml flask is filled with 0.80 mol of I₂ and 2.0 mol of HI. This reaction becomes possible: H₂(g) +I₂(g) ⇌ 2HI(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 H₂. You can leave out the M...
Suppose a 500. mL flask is filled with 1.3 mol of H,O, 1.6 mol of CO2 and 0.80 mol of H. This reaction becomes possible: CO(g) +H2O(g) + CO2(g) +H2 (8) 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...
Suppose a 250 ml flask is filled with 1.4 mol of O, and 0.60 mol of SO,. This reaction becomes possible: 250 (8)+0,(0) - 250 (8) 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...
Suppose a 500. ml flask is filled with 0.90 mol of NO,, 0.10 mol of CO and 0.50 mol of NO. The following reaction becomes possible: NO2(g) +CO(g) = NO(g) + CO2(g) The equilibrium constant K for this reaction is 0.172 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM xs ?
Suppose a 500. mL flask is filled with 0.90 mol of OC1,, 0.20 mol of BroCl and 1.4 mol of BrCl. The following reaction becomes possible: Br2(g) +OC12(g) =BroCl(g) +BrCl(g) The equilibrium constant K for this reaction is 0.798 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. IM xs ?