Suppose a 500 ml flask is filled with 0.30 mol of CH4, 0.60 mol of H20...
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 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...
Song up a reaction Suppose a 500 ml flask is filled with 0.90 mol of CH4, 1.9 mol of H,S and 0.50 mol of CS,. This reaction becomes possible: CH,()+2H,S(g) -CS,() +4H, (®) 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 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 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 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 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 500. mL flask is filled with 0.40 mol of CO, 0.60 mol of NO and 0.70 mol of CO2. The following reaction becomes possible: NO2(g) +CONO( CO2() The equilibrium constant K for this reaction is 9.06 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. Џи
where did the 1.4, 1.6, 0.60 come from? QUESTION Suppose a 500 ml flask is filled with 0.70 mol of NO,, 0.80 mol of CO and 0.30 mol of NO. The following reaction becomes possible NO2(g) + CO(g) - NO(g) + CO2(g) The equilibrium constant K for this reaction is 0.986 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. initial change equilibrium [NO2][co] [no] [CO2] | 1.4 1.6 0.600...