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Consider the following chemical equilibrium. K.(25°C) 10.0 If a sealed 250 mL flask contains 4.00 mol...
A 500.0-mL sealed flask contains 0.060 mol of neon and 0.050 mol of argon at 25°C. Select the correct partial pressures for each of the gases. R=0.0821 L.atm/K-mol Check all that apply. Pe= 5.4 atm P = 2.9 atm P.-2.9 atm = 5.4 atm Ar PA = 2.4 atm Do you know the answer?
Suppose a 250. ml flask is filled with 0.50 mol of H, and 0.40 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) = 2HCl (g) The equilibrium constant K for this reaction is 5.61 at the temperature of the flask. Calculate the equilibrium molarity of Cl. Round your answer to two decimal places. TOM xo?
Suppose a 250. ml flask is filled with 1.7 mol of H, and 0.30 mol of Cly. The following reaction becomes possible: H2(g) + Cl2(g) - 2HCI(g) The equilibrium constant K for this reaction is 6.15 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places. OM xo?
In a sealed 250 mL flask, 0.0403 g of liquid water is in equilibrium with its vapor at 70°C. Calculate the percentage of the total mass of water that is in the vapor phase. Water data: ρ = 1.00 g mL–1; p*(70°C) = 0.308 atm
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 2.0 mol of NO and 0.30 mol of NO . The following reaction becomes possible: NO(g) + NO(g) - 2NO() The equilibrium constant K for this reaction is 0.662 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places. x ?
Suppose a 250 mL flask is filled with 1.6 mol of NO and 0.40 mol of NO2. The following reaction becomes possible: NO3 (g) + NO (g) = 2NO2 (g) The equilibrium constant K for this reaction is 0.253 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 1.8 mol of Cl2 and 0.60 mol of HCl. The following reaction becomes possible: H(+Cl()2HCI) The equilibrium constant K for this reaction is 8.25 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.30 mol of H2 and 1.3 mol of HI. The following reaction becomes possible: H2(8)+12)2HIg) The equilibrium constant K for this reaction is 0.254 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places. Ar
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.