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 and the concentration of Brris -1 0.174 mol L1 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 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G

A chemical engineer is studying the following reaction: 2 NO(g)+2H2(g) → N,(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.17. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound pressure expected change in pressure NO 3.80 atm f increase CI decrease (no change) H2 5.43 atm f increase I decrease (no change) А N2 7.72 atm f increase I decrease (no change) H,0 3.07 atm f increase C+ decrease (no change) NO 4.19 atm f increase I decrease (no change) H, 5.64 atm f increase I decrease (no change) В N2 6.22 atm f increase I decrease (no change) H,0 1.83 atm f increase I decrease (no change) NO 3.39…

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)

The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.400 M , [B] = 1.40 M , and [C] = 0.300 M. The following reaction occurs and equilibrium is established: %3D %3D A + 2B = C At equilibrium, [A] = 0.270 M and [C = 0.430 M. Calculate the value of the equilibrium constant, K. Express your answer numerically. • View Available Hint(s) ΑΣφ Kc =

LRererencesj Isoidan 1 Use the References to access important values if needed for this question. Consider the following equilibrium system at 844 K. 2HI(8) 2 H2 (g) + L (g) If an equilibrium mixture of the three gases at 844 K contains 0.196M HI, 3.37 × 10-2 M H2, and 2.80 × 10- M I2, what is the value of the equilibrium constant K?

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.

At a certain temperature, the equilibrium constant k for the following reaction is 6.3 x 10*: NO,(g) + CO(g) = NO(g) + CO,(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 1.1 mol of NO2 and 1.1 mol of Co. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. There will be very little NO and CO2. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = NO(9)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = | 3 NO,(9)+3CO(9) 3 NO(9)+3CO2(9)