I. Below is some data on equilibrium constants at varying pressures and different temperatures. P/P 0.000197 0.001 0.01 0.1 1 10 20 30 40 50 G Urea (Scheme 1) (T=413.15 K) 3.705-107 1.434 106 1.428.105 1.423 10² 1.417 1.411-10-² 3.525-10-3 1.566-10-3 0.88-10-3 0.563 10-3 G CO₂ (Scheme 2) (T=453.15 K) 2.19 10-9 1.11.10-8 1.11.10-7 1.11.10-6 1.11.10-5 1.11.10 4 2.22-10-4 3.33 10 4 4.44-10-4 5.55-10-4 P/P is the ratio of reaction pressure to the standard pressure 101,325 Pa. How does each reaction's equilibrium change with pressure? J. Propose a set of conditions for reaction 2, including temperature, pressure, and starting amounts, that will maximize the CO₂ reacted. Use an argument with the claim-evidence- reasoning structure described above. Claim should include conditions, evidence can be data provided plus any extra calculations/models you did, and reasoning should explain to me how the data support your claim.

Consider the reaction: P(s) + 3/2Cl₂ (9) ⇒ PCls (g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: $ 4 P(s) +5/2C1₂ (9) PC15 (9) K1 PC13 (9) + Cl₂ (g) =PC15 (9) K₂ Submit Answer For answers with both a subscript and a superscript, enter the subscript first. For example, enter K? If the first equilibrium constant should be squared. K = 000 000 F4 R F Show Hint % 5 Retry Entire Group 9 more group attempts remaining [Review Topics] [References] Use the References to access important values if needed for this question. F5 T Cengage Learning Cengage Technical Support G A 6 MacBook Air F6 Y H & ✓ 7 ◄◄ F7 U * 8 J F8 ( 9 ►► K F9 O ) DIO 1108 chat 0 L F10 - P - ^ Previous F11 SAVAGE X FENTY... { + = Next> Save and Exit F12 11 G

Consider the reaction: 12(g) =21(g) The equilibrium constant, Kc, for this reaction is 3.76 x 10-3 at T = 1000 K. Initially, 1.36 moles of 12 is placed into a 5.00 L reaction flask at T = 1000 K. What is the equilibrium concentration of I? Input your answer in units of M (molarity) to 3 decimal places. Your Answer: 4

A mixture of ammonia, nitrogen, and hydrogen was allowed to come to equilibrium at 900K. 2NH3 ⇌ 2H2 + N2        Kc = 0.0076. An analysis of the mixture at equilibrium revealed 0.31 M of H2 and 1.8 M of NH3. Determine the equilibrium concentration of N2 (in M) in this mixture. (use 2 significant figures)

Calculate the value of Kc.

For the reaction 12(g) +Br₂(g) →21Br(g) Ke=280 at 150 °C. Suppose that 0.520 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150 °C. Esc Type here to search WE in R ▼ What is the equilibrium concentration of I₂? Express your answer in moles per liter to three signifi IVE ΑΣΦ [12] = 0.012 Submit Previous Answers Request Answer * Incorrect; Try Again; 7 attempts remaining Part C What is the equilibrium concentration of Br₂? Express your answer in moles per liter to three significant figu ΕΧΕΙ ΑΣΦ Br₂ = 0.0120 Submit Previous Answers Request Answer ? 8 M