The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl (g) → 2 NO (g) + Cl2 (g) Suppose that 0.730 mol NOCl is placed in a 2.00-L flask at a given temperature. When equilibrium has been established, it is found that the concentration of NO is 0.0906 M. Calculate the equilibrium constant for this reaction.
The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl...
2. The compound NOCI decomposes to nitric oxide and chlorine according to the following equation: 2 NOCI (g) 2 NO (g+ Cl (g) Suppose that 0.480 mol NOCI is placed in a 5.00-L flask at a given temperature. When equilibrium has been established, is found that the concentration of NO is 0.0196 M. Calculate the equilibrium constant for this reaction.
The reaction between nitric oxide (NO) and chlorine (Cl2) to form nitrosyl chloride (NOCl) was found to occur as an elementary reaction as follows: 2 NO (g) + Cl2 (g) à 2 NOCl (g) A table of the concentrations and initial rates data is shown below: [ NO ]0 (M) [ Cl2 ]0 (M) rate = - D[Cl2]/ Dt (M / min) Run 1 0.10 0.10 0.18 Run 2 0.10 0.20 0.36 Run 3 0.20 0.20 1.44 The order for Cl2 in this reaction is: (a) 1 (b) 45 (c) 2 (d) 180
3. Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2(g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.180 mol N2 and 0.650 mol O2 are mixed in a 4.00-L reaction vessel. What will be the concentrations of N2, 02, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small-less than 10% of the starting...
3. Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.280 mol N2 and 0.120 mol O2 are mixed in a 3.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the...
When heated, colorless dinitrogen tetraoxide, N2O4(g), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204 (g) + 2 NO2 (g) Suppose that 2.00 mol of N204(g) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K, for this reaction at 407 K. 3.80 2.00 0.500 0.263 0.525
19. Compound A decomposes to B and C according to the following equation: 2A(g) > B(g) + 2 (g) At 100 Celcius, 1.45 mol of A were placed in a 5.00 L container, and the reaction was allowed to proceed. After equilibrium was established, it was found that 67.9% of A had decomposed. What is the value of Kc for this reaction at 100 Celcius? a. 0.371 b. 0.343 c. 0.441 d. 0.407 e. 0.609
When heated, colorless dinitrogen tetraoxide, N204(8), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204(g) 42 NO2 (g) Suppose that 2.00 mol of N204(8) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K., for this reaction at 407 K. 0.500 O 0.525 2.00 0.263 3.80
21. Nitric oxide gas reacts with chlorine gas according to the equation: The following data were obtained for this reaction initial rate mol(I br. initial [NO] initial [Cl2] 1.19 0.50 0.50 4.19 1.00 0.50 1.00 1.00 9.59 1.50 32.27 1.50 Which of the following rate laws is consistent with these data? A. Rate kINO1 1/2 C. Rate kINO][C12] D. Rate kINO]2[Cl2] E. Rate k[NO] [Cl212
Nitric oxide (NO) reacts with chlorine gas (Cl) to form nitrosyl chloride (NOC) according to the reaction below: 2 NO(g) + C12()=2 NOCI(g) Kp = ? at 700 K A rigid vessel initially contains equimolar amounts of NO and C1, (and nothing else) at 700 K and a total pressure of 2.00 bar. After the system reaches equilibrium at 700 K, the total pressure is found to be 1.84 bar. What is the value of the equilibrium constant Kp? A)...
points Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3C12() SC12(Ⓡ) + CC446) When 1.14 mol of CS2 and 4.80 mol of Cl2 are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.650 mol of CC14. How many moles of Cl2 are present at equilibrium? a. 0.490 mol b. 3.50 mol OC 0.650 mol d. 1.43 mol e. 2.85 mol