A student ran the following reaction in the laboratory at 1098 K: 2 S03 (g) 2 So2 (g) + 02 (g) When she introduced 8.28x10-2 moles of SO3 (g) into a 1.00 liter container, she found the equilibrium concentration of O2 (g) to be 1.83x102 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

During an experiment, O.257 mol of H2 and 0.257 mol of I2 were placed into a 1.28 liter vessel where the reaction H2(g) + 12(g) 2 2HI(g) came to equilibrium. For this reaction, Kc = 49.5 at the temperature of the experiment. What were the equilibrium concentrations of H2, 12, and HI? [H2] = M %3D [12] = M [HI] = i M

A student ran the following reaction in the laboratory at 1097 K: 2SO3(g)2SO2(g) + O2(g) When she introduced 0.0921 moles of SO3 (g) into a 1.00 liter container, she found the equilibrium concentration of O₂ (g) to be 0.0198 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

A student ran the following reaction in the laboratory at 672 K: 2NH3(g)     N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

A student ran the following reaction in the laboratory at 431 K: PCI 5(9) PC13(g) + Cl₂(9) When she introduced 2.02 moles of PCI5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.08x10-² M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.

A student ran the following reaction in the laboratory at 282 K: 2CH2C12(g)=CH4(g)+ CCI4(g) When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =

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…