The reaction 2NO_2 (g) + F_2(g) rightarrow 2NO_2 F(g) has a second order rate la

Question

The reaction 2NO_2 (g) + F_2(g) rightarrow 2NO_2 F(g) has a second order rate law, rate = k[NO_2][F_2]. Suggest a mechanism that is consistent with this rate law. A sample of HI (9.30 Times 10^-3 mol) was placed in empty 2.00 L container at 1000 K. After equilibrium was reached the concentration of I2 was 6.29 Times 10^-4 M. Calculate the K_c at 1000 K for the reaction H_2 (g) + I_2 (g) doubleheadarrow 2HI(g) Hydrogen Iodide decomposes slowly to H_2 and I_2 at 600 K. The reaction is second order in HI and the rate constant is 9.7 Times 10^-6 M^-1 s^-1. Assume the initial concentration of HI is 0.100 M: What is its molarity after a reaction time of 6.00 days? What is the time (in days) when the HI concentration reaches a value of 0.085 M? Calculate the pH and the percent dissociation in 1.5 M HNO_2 (K_a = 4.5 Times 10^-4). An equilibrium mixture of PCl_5, PCl_3, and Cl_2 at a certain temperature contains 8.3 Times 10^-3 M PCl_5, 1.5 Times 10^-2 M PCl_3, and 3.2 Times 10^-2 M Cl_2. Calculate the equilibrium constant Kc for the the reaction PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2 (g) Calculate the pH of solution prepared by mixing 100.0 mL of 2.0 Times 10^-3 M HCl and 400.0 mL of 1.0 Times 10^-3 M HClO_4 (assume that the volumes are additive). Calculate the pH of 0.250 L of a 0.36 M Formic acid HCO_2H-0.30 M Sodium formate NaCO_2H buffer before and after the addition of 0.0050 mol of NaOH and 0.0050 mol of HCl. Assume that volume remains constant (K_a for HCO_2H = 1.8 Times 10^-4). Consider the titration of 40.0 mL of 0.25 M HF(ka = 3.5 Times 10^-4) with 0.2 M NaOH. How many milliliters of base are required to reach the equivalence point? What is the pH after the addition of 10.0 mL of base? What is the pH halfway to the equivalence point? Calculate the molar solubility of SrF_2 (K_ap = 4.3 Times 10^-9) in: 0.010 M Sr(NO_3)_2 0.010 M NaF Will a precipitate of CaCO_3 form if a 250 mL solution with [Ca^2+] = 8.0 Times 10^-4 M is treated with 0.10 mL of 2.0 Times 10^-3 M Na_2CO_3 ? K_ap for CaCO_3 = 5.0 Times 10^-9 Calculate Delta G at 25 degree C for the reaction 2SO_2(g) + O_2(g) rightarrow 2SO_3(g) Delta G degree = -148Kj under the following set of pressures: 100atm SO_2, 100atm O_2, 1.0 atm SO_3 Consider a galvanic cell based on the reaction 2Fe^2+(aq) + Cl_2 (g) rightarrow 2 Fe^3+ (aq) + 2Cl^- (aq) Calculate the cell potential at 25 degree C when [Fe^2+] =1.0 M, [Fe^3+] = 1.0 Times 10^-3 M, [Cl^-] = 3.0 Times 10^-3 M and PCl_2 = 0.50 atm.

Explanation / Answer

question 2:

H2 + I2 = 2HI

Concentration of HI = 9.3x10-3 / 2 = 0.00465 M

If concentration in equilibrium of I2 is 6.29x10-4 means that H2 has the same concentration, so Kc is:

Kc = (HI)2 / (H2)(I2)
Kc = (0.00465 - 2(6.29x10-4)) / (6.29x10-4)2
Kc = 0.005908 / 3.956x10-7
Kc = 1.493x104

3. If this is a reaction of second order, the expressio n to use is the following:

1/A = 1/Ao + kt for at t = 6 days (6 days * 24 h/day * 3600 s/h = 518400 s)

1/A = 1/0.1 + 518400*9.7x10-6
1/A = 10 + 5.0285
A = 0.0665 M

For part b) t would be:

1/0.085 - 1/0.1 = 9.7x10-6t
1.7647/9.7x10-6 = t
t = 181927.84 s

The other questions post them in another post. Hope this helps

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