A student measures the reaction H₂(g) + Cl₂(g) <=> 2 HCl(g) concentrations at a few different temperatures and obtains the equilibrium constant. The student wants to use the van't Hoff equation to roughly determine the reaction enthalpy assuming that it does not change over the region of interest. T(K) 300 500 4x1018 4x1031 Keq So the student plots the data in the InK vs 1/T diagram and obtains a linear fitting shown below: 80 8382 60 240 20 0 y-22585x-24632 0 (¹) 0.002 0.004 1000 4×108 What is the reaction enthalpy value obtain from this figure? kJ/mol 3sig fig. (hint, rearrange the equation so that you can clearly see the slop and the intercept)

For the  reaction 3H2(g)+N2(g)⇌2NH3(g) at 225 ∘C the equilibrium contant  is 1.7×10 ^2. If the equilibrium mixture contains 0.19 M H2 and 0.015 M N2, what is the molar concentration of NH3? Express your answer to two significant figures and include the appropriate units.

At 100 °C, Keg = 1.5E8 for the reaction: CO(g) + Cl2(g) - COCI2(g) Using appropriate approximation, calculate the partial pressure of CO at 100 °C at equilibrium in a chamber that initially contains COCI2 at a pressure of 0.302 bar.

Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)

The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ

Consider the hypothetical reaction A(g) 2B(g). A flask is charged with 0.74 atm of pure A. after which it is allowed to reach equilibrium at 0 °C. At equilibrium the partial pressure of A is 0.37 atm Part A What is the total pressure in the flask at equilibrium? Express your answer using two significant figures. VS ΑΣΦ 4 P₁ = Submit Part B What is the value of Kp? Express your answer using two significant figures. K₂= Submit Part C Request Answer |VL ΑΣΦ Submit Request Answer What could we do to maximize the yield of B? → Request Answer [w] ? O Doing the reaction in a larger flask maximizes the yield of B. O Doing the reaction in a smaller flask maximizes the yield of B. atm

For the equilibrium reaction.   2IBr (g) I2 (g) + Br2 (g) Kc=.0085.  If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components.   Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.

Keq for a Gas-Phase Reaction A 5.00-L vessel contained 9.49×102 mol of gaseous PCI3, 8.03×102 mol of gaseous PCI5, and 8.21x102 mol of Cl2 gas at equilibrium at 233°C. Calculate the value of Keg (expressed in terms of the molar concentrations) for the reaction PCI3(g) + Cl2(g) = PCI5(g) (No units required.)