This law established the requirement for “full and open competition” means that all responsible sources may submit proposals or bids.

Consider the following equilibrium:            N2(g) + 3 H2(g) ⇌ 2 NH3(g) The following concentrations were measured at equilibrium: [N2] = 0.100 M, [H2] = 0.200 M and [NH3] = 2.36 x 10-1 M for the following reaction at 350oC Calculate the equilibrium constant. Enter your answer (3 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (2 pts). ⚠️Work required for credit.

Consider the following reaction: I2(g) +  H2(g)  ⇌   2HI(g) A closed system initially containing 1.00 × 10–3 M H2 and 2.00×10–3 M I2 at 500oC is allowed to reach equilibrium. The equilibrium mixture shows that the concentration of HI is 1.90 × 10–3 M. Build a RICE table and  calculate Kc Enter your answer (3 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (2 pts). ⚠️Work required for credit.

The Ka of lactic acid, CH3CH(OH)CO2H, a weak monoprotic acid found in the blood after strenuous exercise, is 1.36 × 10-4. Build a RICE table or write the correct expression for Ka and calculate the pH of 0.222 M solution of lactic acid. Enter your answer (3 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (3 pts). ⚠️Work required for credit.  

The Ka of hypochlorous acid (HClO) is 3.00×10-8 Build a RICE table or write the correct expression for Ka and calculate the pH of 0.0200M solution of hypochlorous acid. Enter your answer (3 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (3 pts). ⚠️Work required for credit.

Determine the molarity of HI when the following reaction reaches equilibrium. Other equilibrium concentrations are found to be as follows: [HCl] = 1.6 × 10-3 M, [Cl2] = 0.0012 M. The value of Kc for this reaction is 2.8 × 1031. 2HI(g) + Cl2(g) ⇌ 2 HCl(g) + I2(s) Enter your answer. After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment. ⚠️Work required for credit.

The Ka of acetic acid (CH3COOH) is 1.8×10-5 Build a RICE table or write the correct expression for Ka and calculate the pH of 0.70M aqueous solution of acetic acid. Enter your answer (3 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (3 pts). ⚠️Work required for credit.

Consider the following equilibrium:      3 H2(g) + CO(g)  ⇌  CH4(g) + H2O(g) The following concentrations were measured at equilibrium: [CO] = 0.152 M, [H2] = 0.157 M, [CH4] = 0.0478 M and [H2O] = 0.0478 M for the following reaction at 1200oK. Calculate the equilibrium constant. Enter your answer (3 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (2 pts). ⚠️Work required for credit.

The three positions of preparing a negotiation objective are:

Calculate Kp for the following generic reaction at 300K:         2AB(g)⇌ 2A(g) + B2(g)  Kc=1.5X10-3 Enter your answer (1 pts). After submitting this exam, upload your matching work in the Midterm 2: Required Work, Partial Credit, and Extra Credit assignment (2 pts). ⚠️Work required for credit.