Question

9. For the following reaction, ?P(C6H14)/?t was found to be -6.6 × 10?¹ atm/s. C6H14(g) ? C6H6(g) + 4H2(g) Determine ?P(H2)/?t for this reaction at the same time. A. 4.1E-2 atm/s B. 1.6E-1 atm/s C. 2.6E0 atm/s D. 6.6E-1 atm/s E. 1.1E1 atm/s 10. A chemical reaction of the general type A ? 2B is first-order, with a rate constant of 2.99 × 10?³ s?¹. Calculate the half-life of A and the time needed for the concentration of A to fall from 0.108 mol L?¹ to 0.058 mol L?¹. A. 3.34E2 s; 1.67E1 s B. 1.67E2 s; 1.80E2 s C. 2.32E2 s; 2.08E2 s D. 2.32E2 s; 1.67E1 s E. 3.34E2 s; 2.08E2 s 11. The reaction CH3NC(g) ? CH3CN(g) is first-order with respect to methyl isocyanide, CH3NC. If it takes 28.5 minutes for exactly 58.8% of the initial amount of methyl isocyanide to react, what is the rate constant in units of min?¹? A. 1.91E-2 min?¹ B. 2.04E-2 min?¹ C. 1.47E-2 min?¹ D. 4.85E-2 min?¹ E. 3.04E-2 min?¹ 12. Consider the reaction N2(g) + O2(g) ? 2NO(g), for which Kc = 0.10 at 2,000°C. Starting with initial concentrations of 0.073 M of N2 and 0.073 M of O2, determine the equilibrium concentration of NO. A. 9.97E-3 M B. 5.35E-3 M C. 6.96E-3 M D. 7.30E-2 M E. 1.99E-2 M

          9. For the following reaction, ?P(C6H14)/?t was found to be -6.6 × 10?¹ atm/s.
C6H14(g) ? C6H6(g) + 4H2(g)
Determine ?P(H2)/?t for this reaction at the same time.
A. 4.1E-2 atm/s
B. 1.6E-1 atm/s
C. 2.6E0 atm/s
D. 6.6E-1 atm/s
E. 1.1E1 atm/s

10. A chemical reaction of the general type A ? 2B is first-order, with a rate constant of 2.99 × 10?³ s?¹.
Calculate the half-life of A and the time needed for the concentration of A to fall from 0.108 mol L?¹ to 0.058 mol L?¹.
A. 3.34E2 s; 1.67E1 s
B. 1.67E2 s; 1.80E2 s
C. 2.32E2 s; 2.08E2 s
D. 2.32E2 s; 1.67E1 s
E. 3.34E2 s; 2.08E2 s

11. The reaction CH3NC(g) ? CH3CN(g) is first-order with respect to methyl isocyanide, CH3NC. If it takes 28.5 minutes for exactly 58.8% of the initial amount of methyl isocyanide to react, what is the rate constant in units of min?¹?
A. 1.91E-2 min?¹
B. 2.04E-2 min?¹
C. 1.47E-2 min?¹
D. 4.85E-2 min?¹
E. 3.04E-2 min?¹

12. Consider the reaction N2(g) + O2(g) ? 2NO(g), for which Kc = 0.10 at 2,000°C. Starting with initial concentrations of 0.073 M of N2 and 0.073 M of O2, determine the equilibrium concentration of NO.
A. 9.97E-3 M
B. 5.35E-3 M
C. 6.96E-3 M
D. 7.30E-2 M
E. 1.99E-2 M

9. For the following reaction, ?P(C6H14)/?t was found to be -6.6 × 10?¹ atm/s.
C6H14(g) ? C6H6(g) + 4H2(g)
Determine ?P(H2)/?t for this reaction at the same time.
A. 4.1E-2 atm/s
B. 1.6E-1 atm/s
C. 2.6E0 atm/s
D. 6.6E-1 atm/s
E. 1.1E1 atm/s

10. A chemical reaction of the general type A ? 2B is first-order, with a rate constant of 2.99 × 10?³ s?¹.
Calculate the half-life of A and the time needed for the concentration of A to fall from 0.108 mol L?¹ to 0.058 mol L?¹.
A. 3.34E2 s; 1.67E1 s
B. 1.67E2 s; 1.80E2 s
C. 2.32E2 s; 2.08E2 s
D. 2.32E2 s; 1.67E1 s
E. 3.34E2 s; 2.08E2 s

11. The reaction CH3NC(g) ? CH3CN(g) is first-order with respect to methyl isocyanide, CH3NC. If it takes 28.5 minutes for exactly 58.8% of the initial amount of methyl isocyanide to react, what is the rate constant in units of min?¹?
A. 1.91E-2 min?¹
B. 2.04E-2 min?¹
C. 1.47E-2 min?¹
D. 4.85E-2 min?¹
E. 3.04E-2 min?¹

12. Consider the reaction N2(g) + O2(g) ? 2NO(g), for which Kc = 0.10 at 2,000°C. Starting with initial concentrations of 0.073 M of N2 and 0.073 M of O2, determine the equilibrium concentration of NO.
A. 9.97E-3 M
B. 5.35E-3 M
C. 6.96E-3 M
D. 7.30E-2 M
E. 1.99E-2 M

Added by Tamara K.

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