The equilibrium constant, Ke, for this reaction is 57. H2 (9) + I2(9) = 2HI(9) If the equilibrium mixture contains 0.020 M I2 and 0.033 M HI, what is the molar concentration of H2 ? Express your answer to two significant fiqures and includo tho anpronrinto unito

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.

Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). (a) O,(g) 503(s K. = 8.70 × 10-9 |× 10 K. = (Enter your answer in scientific notation.) (b) 30,(g) 5 203(g)

For the reaction  3 A --> B + 2C, 3.60 mol A is placed in a 3.00 L vessel. At equilibrium the concentration of B is 0.300 M. Determine the value of the equilibrium constant, Kc.

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700 M, B] = 0.950 M , and [C = 0.500 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.510 Mand C = 0.690 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically.

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?

A student ran the following reaction in the laboratory at 279 K: 2CH,Cl,(g)CHĄ(g) + CC14(g) When she introduced 8.03x102 moles of CH,Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of CCl(g) to be 3.76x102 M. Calculate the equilibrium constant, K, she obtained for this reaction. K =|

Enter your answer in the provided box. Given the reaction 2HI(g) 2 H2(g) + I,(g) Kea = 1.0 × 101 eq A sample mixture of HI, H,, and I, at equilibrium, was found to have [H2] = 3.0 × 10¬' M and HI] = 7.6 x 10 M. Calculate the molar concentration of I, in the equilibrium mixture. [L] =

A chemical engineer is studying the following reaction: CH₂(g) + 2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³. р The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound CH4 H₂S CS₂ H₂ CHA H₂S CS₂ H₂ pressure 5.65 atm 3.56 atm 5.77 atm 7.93 atm 4.69 atm 1.62 atm 6.73 atm 11.81 atm OO expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase olo ↓decrease ↓decrease ↓ decrease ↓decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no change) (no…

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