MISSED THIS? Read Section 16.8 (Page); Watch KCV 16.8, IWE 16.12. Consider the reaction Br2(g) + Cl₂(g) = 2BrCl(g) K₂1.11 x 10-4 at 150 K A reaction mixture initially has a Br₂ partial pressure of 753 torr and a Cl₂ partial pressure of 687 torr at 150 K. Part A Calculate the equilibrium partial pressure BrCl. Express your answer in torr to three significant figures. for Part for Pant A do for Part redo for Part A refor Part A keyboar P(BrCl) 7.38 Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining

A student ran the following reaction in the laboratory at 377 K: CH₂(g) + CCL (9) ⇒ 2CH₂Cl2 (9) When she introduced 0.0391 moles of CH4 (g) and 0.0708 moles of 14 CCl4 (g) into a 1.00 liter container, she found the equilibrium concentration of CCl4 (g) to be 0.0623 M. Calculate the equilibrium constant, Ko, she obtained for this reaction. Kc =

The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.366 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K

The equilibrium constant, Ke, for the following reaction is 7.00 x 10-5 at 673 K. to access important values if needed for this question. NH₂I(s) ⇒ NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.33 L container at 673 K contains 1.71 mol of NH₂I(s) and 0.445 mol of NH3, the number of moles of HI present is mol.

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react according to the following reaction. PCI2(g) + Cl2(g) ⇌ PCI5(g) The equilibrium constant for the reaction is Kc = 43.7 at 130 °C. If 0.587 mo/ of phosphorus trichloride is added to 0.423 mol of chlorine in a 1.26-L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of chlorine? Report your answer to THREE significant figures.

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…

The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.0×10^-3. If the equilibrium mixture contains [NO2] = 0.055 M , what is the molar concentration of N2O4?

The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)Calculate the equilibrium concentration of HCl when 0.227 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K.[HCl] =  M