At 1285 °C, the equilibrium constant for the reactionBr2(g) ⇌ 2 Br(g) is Kc = 1.04 x 10-3. A 0.200-L vesselcontaining an equilibrium mixture of the gases has 0.245 gBr2(g) in it. What is the mass of Br(g) in the vessel?

At a particular temperature, K = 1.7 × 10-7 for the following balanced reaction: 2CO₂(g) → 2CO(g) + O2(g) In an experiment in which 2.0 mol of CO₂ is placed in a 2.0-L vessel, what are the equilibrium concentrations of all gases? [CO₂] = [Co] = [0₂] = ΣΣΣ

Hydrogen gas and bromine gas are mixed in a sealed container at 250°C and allowed to reach equilibrium. H2(g) + Br2(g) = 2HB1(g) The equilibrium constant for this reaction at 250°C is 65.5. At equilibrium, the concentration of H2 is 0.0510 mol L*1 and the concentration of Brris 0.174 mol L-1 at 250°C. (i) Write the equilibrium constant expression for the above reaction. (ii) Calculate the concentration of HBr in the equilibrium mixture at 250°C (iii) Explain what happens to the concentration of HBr you calculated in (ii) above if the pressure of the equilibrium mixture is increased.

Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

-2 The equilibrium constant K,, for the following reaction is 7.73×10atmat 350°C. What is the value of K. for the reaction at the same temperature? N2(g) +3H2(g)→ 2NH3(g)

At 800 K, the equilibrium constant for the following reaction is Kc = 3.1×10^−5: I2(g)⇌2I(g) If an equilibrium mixture in a 10.0-L vessel contains 2.69×10^−2g  of I, how many grams of I2 are in the mixture? Express your answer in grams to two significant figures.

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N, (g) + 3 H, (g) = 2 NH3 (g) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.

At 454 K, Al,Cl6(g) reacts to form Al;Cl,(g) according to the equation 3 Al,Cl,(g) = 2 Al;Cl,(g) In an experiment at this temperature, the equilibrium par- tial pressure of Al,Cl(g) is 1.00 atm and the equilibrium partial pressure of Al;Cl,(g) is 1.02 × 10-2 atm. Compute the equilibrium constant of the preceding reaction at 454 K.

The equilibrium constant, Kc, for the following reaction is 1.20\times 10 - 2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.331 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K.