homework problems: Place the final answer in the box. 1. Given the reaction N2(g) + 3H2(g)  2NH3(g) The rate H2 is reacting is 0.074 M/s 2. a. What is the rate NH3 is formed? b. What is the rate N2 is reacting? a. Determine the rate law for the following reaction using the data provided. F2(g) + 2 ClO2(g) → 2 FClO2(g) [F2]i (M) [ClO2]i (M) Initial Rate (M/s) 0.10 0.010 0.10 0.040 1.2 x 10-2 4.8 x 10-2 0.20 0.010 2.4 x 10-2 b. Determine the value of k. Determine the value of k c. What is the initial rate if [F2] = 0.010 M and [ClO2] = 0.020 M? Determine the value of k Initial rate of disappearance of X (M/s) [X] 3. Given the reaction X + Y  Z and the data table below. Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 a. [X] 0.10 0.20 0.40 0.20 0.40 [Y] 0.50 0.30 0.60 0.60 0.30 Determine the reaction order for X and Y and overall reaction order. X Y Deter mine the value of k Deter mine the value of k Overall Deter mine the value of k Initial rate of Initial rate of Initial rate of disappearancedisappearance disappearance of X (M/s) of X[X] (M/s) [Y] of X[X] (M/s) 0.147 0.147 0.1 0.50.147 0.1 0.127 0.127 0.2 0.30.127 0.2 4.064 4.064 0.4 0.64.064 0.4 1.016 1.016 0.2 0.61.016 0.2 0.508 0.508 0.4 0.30.508 0.4 b. [Y] 0.5 0.3 0.6 0.6 0.3 [X] 0.1 0.2 0.4 0.2 0.4 Determine the rate of disappearance when [X] =0.30 M and [Y] = 0.40 M. Determine the value of k Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 [X] 0.1 0.2 0.4 0.2 0.4 4. Given the reaction A  B with a rate of 1.6 x 10-2 M/s at [A] = 0.35 M. a. Calculate the rate constant k for 1st order reaction. Determine the value of k b. Calculate the rate constant k for 2nd order reaction. Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 [X] 0.1 0.2 0.4 0.2 0.4 Determine the value of k 5. Given the 1st order reaction 4PH3(g)  P4(g) + 6H2(g). a. Calculate the rate constant if the half-life of the reaction is 3.50 sec at 680oC. Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 [X] 0.1 0.2 0.4 0.2 0.4 Determine the value of k b. Calculate the time required for 95% of PH3 to decompose. Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 Determine 0.508the value of k Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 [X] 0.1 0.2 0.4 0.2 0.4 [X] 0.1 0.2 0.4 0.2 6. The rate constant for the second-order reaction below is 0.54/M . s. 2NO2(g)  2NO(g) + O2(g) a. How long would it take for the concentration of NO2 to decrease from 0.62 M to 0.28 M? Determine the value of k b. Calculate the half-lives at these two concentrations. Initial rate of Initial rate o disappearance disappearan of X (M/s) of X (M/s) 0.147 0.147 0.127 0.127 4.064 Determ 4.064 Determ 1.016 ine the1.016 ine the 0.508 value0.508 value of k of k Initial rate of Initial rate of disappearancedisappearance of X (M/s) of X (M/s) [X] 0.147 0.147 0.1 0.127 0.127 0.2 4.064 4.064 0.4 1.016 1.016 0.2 0.508 0.508 0.4 7. For a given reaction, the rate is 1.50 x 103 faster at 250 oC than 150 oC (at the same concentrations). Calculate the activation energy for the reaction. Determine the value of k Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 8: The rate constant of a first order reaction is 4.60 x 10-4 /s at 350 oC. If the activation energy is 104 kJ/mole, calculate the temperature at which its rate constant is 8.80 x 10-4 /s. Determine the value of k Initial rate of Initial rate of disappearance disappearance of X (M/s) of X (M/s) 9: If a reaction has a rate of 2.0 x 102 atm/min at 27 oC but only 39.6 atm/min at 5 oC (at the same 0.147 0.147 0.127 0.127 concentrations), what is the activation energy of this reaction? 4.064 4.064 1.016 1.016 Determine the value 0.508 0.508 of k Initial rate of disappearance of X (M/s) 0.147 0.127 4.064 1.016 0.508 Initial rate disappeara of X (M/ 0.147 0.127 4.064 1.016 0.508
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