Chem 102 Final Exam Study Guide Graded A+

The average rate of appearance of [NH3] is 0.215 M/s. Determine the average rate of disappearance of [H2]. N2(g) + 3H2(g) - 2NH3(g) - Answer--0.323 M/s Use the following experimental data to determine the rate law expression and the rate constant K for the following chemical equation; 2NO(g) + O2(g) - N2O4(g) .100M ~ .100M ~ 1.25 x 10^-4 M/s .200M ~ .100M ~ 5.00 x 10^-4 M/s .100M ~ .200M ~ 2.50 x 10^-4 M/s - Answer-Rate = K[NO]^2[O2] K = 0.125 M^-2 s^-1 Which of the following will give a straight line plot in the graph of ln[A] versus time? A. Zero Order B. First Order C. Second Order D. Third Order - Answer-B. First Order Which of the following units of the rate constant K corresponds to a first order reaction? A. M^1 s^-1 B. s^-1 C. M^-1 s^-1 D. M^-2 s^-1 - Answer-B. s^-1 units = M^1-n * time^-1The initial concentration of a reactant is 0.453M for a zero order reaction. Calculate the final concentration of the reactant after 64.4 seconds is the rate constant K is 0.00137 M/s. - Answer- 0.365M The initial concentration of a reactant is 0.738M for a zero order reaction. The rate constant K is 0.0352 M/min. Calculate the time it takes for the final concentration of the reactant to decrease to 0.255M. - Answer-13.7 min Calculate the rate constant K for a second order reaction if the half life is 243 seconds. The initial concentration of the reactant is 0.325M. - Answer-1.27 x 10^-2 M^-1 s^-1 A reaction has a rate constant of 1.46x10^-3 s^-1 at 298K and 4.33x10^-2 s^-1 at 421K. Calculate the activation energy of this reaction. - Answer-28.7 kJ/mol Which particle is equivalent to an electron? - Answer-Beta particle Identify the missing element. 226/88 Ra - 4/2 He + ? - Answer-222/86 Rn The half-life of Cs-137 is 30.0 years. Calculate the rate constant K for the first order decomposition of isotope Cs-137. - Answer-2.31x10^-2 yr^-1 The half-life of Iodine-131 is about 8.03 days. How long will it take for a 200.0g sample to decay to 25g? - Answer-24.1 days What is the correct equilibrium expression for the reaction shown below? CuO(s) + H2(g) - Cu(s) +H2O(g) - Answer-Kp = [H2O]/[H2] *Any reactant or product in the liquid or solid phase should not be included in the expression for K. Calculate Kp for the following reaction at 298K. Kc = 2.41x10^-2CO(g) + 3H2(g) - CH4(g) + H2O(g) - Answer-4.03x10^-5 [Kp = Kc(RT)^Delta N] Delta N = Sum of product coefficients - Sum of reactant coefficients Use the information below to calculate the missing equilibrium constant Kc of the net reaction. 2CO(g) - 2C(s) + O2(g) K1 = 1.43 x 10^-1 ½ CO2(g) - ¼ O2(g) + ½ CO(g) K2 = 2.35 x 10^-2 C(s) + O2(g) - CO2(g) K3 = ? - Answer-4788 (which rounds to) 4790