OKINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium const... Suppose a 250. ml flask is...
Suppose a 250. ml flask is filled with 1.5 mol of Cl, and 1.3 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl (8) The equilibrium constant K for this reaction is 0.560 at the temperature of the flask. Calculate the equilibrium molarity of H. Round your answer to two decimal places. OM * 5 ?
calculate the equilibrium molarity of NO. round to two decimal
places
Suppose a 250 ml. flask is filled with 0.80 mol of CO, 0.60 mol of NO and 0.20 mol of CO. The following reaction becomes possible: NO,(e)+co(s) - NO(g) +00,() The equilibrium constant for this reaction is 9.16 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. 0м X 5 ?
thank you so much to anyone that is able to help
Suppose a 250 ml flask is filled with 0.50 mol of NO, 1.5 mol of CO and 0.80 mol of CO,. The following reaction becomes possible: NO,(g) +CO(g) NO(g) +co,(g) The equilibrium constant K for this reaction is 0.989 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. UM X 5 ?
Suppose a 250. mL flask is filled with 1.2 mol of Cl₂, 1.8 mol of CHCl₃ and 0.90 mol of HCl. The following reaction becomes possible:Cl₂(g)+CHCl₃(g) ⇌ HCl(g)+CCl₄(g)The equilibrium constant K for this reaction is 0.855 at the temperature of the flask.Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.50 mol of H20, 1.0 mol of Co2 and 1.5 mol of H2. The following reaction becomes possible cog)+H20(g)Co()+H28) The equilibrium constant K for this reaction is 4.10 at the temperature of the flask Calculate the equilibrium molarity of H20. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.1 mol of H₂ O, 1.5 mol of CO₂ and 0.80 mol of H₂. The following reaction becomes possibleCO(g)+H₂ O(g) ⇌ CO₂(g)+H₂(g)The equilibrium constant K for this reaction is 7.29 at the temperature of the flask.Calculate the equilibrium molarity of CO₂. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.8 mol of No₃ and 1.5 mol of NO₂. The following reaction becomes possible: No₃(g) + No(g) ⇄ 2No₂(g) The equilibrium constant K for this reaction is 3.20 at the temperature of the flask. Calculate the equilibrium molarity of No₂. Round your answer to two decimal places.
Suppose a 250. ml flask is filled with 1.6 mol of Cl, and 1.3 mol of HCI. The following reaction becomes possible: H2(g) + Cl2(g) → 2HCI (g) The equilibrium constant K for this reaction is 0.967 at the temperature of the flask. Calculate the equilibrium molarity of C1. Round your answer to two decimal places. OM I ?
Suppose a 250. ml flask is filled with 0.50 mol of CO, 0.60 mol of NO and 2.0 mol of CO2. The following reaction becomes possible: NO2(g) + CO(g) = NO(g) + CO2(g) The equilibrium constant K for this reaction is 3.29 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM x 6 ?
Suppose a 250 ml flask is filled with 0.30 mol of I, and 1.5 mol of HI. The following reaction becomes possible: H2(g) +12(g)=2HI(g) The equilibrium constant K for this reaction is 0.532 at the temperature of the flask. Calculate the equilibrium molarity of 12. Round your answer to two decimal places. Пм x s ?