[6]BONUS: kl -5,5x10-3 3-1 at 315 K, find k2 at 415 Kif Ea - 45.5 kJ/mol.
a. Calculate Ea if k1 = 4.62 x 10 -7 1/Ms at 315 oC and k2 is 2.31 x 10 -4 1/Ms at 678 oC. b. Based on your answer to a, what’s k at 400 oC?
If a reaction with Ea = 83 KJ/mol and k = 2.1x10^-2 s-1 at 150C, what will be the value of k at 210C
Find ΔrG for the following (in kJ mol-1) N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) The conditions for this reaction are: Temp: 298k P - NH3 = 0.95 bar P - H2 = 1.95 bar P - N2 = 1.25 bar NH3(g) ?H ∙(kJ mol-1) = -45.9 ?G ∙(kJ mol-1) = -16.4 S ∙(J K-1 mol-1)192.8 N2(g) ?H ∙(kJ mol-1) = 0 ?G ∙(kJ mol-1) = 0 S ∙(J K-1 mol-1)191.6 H2(g) ?H ∙(kJ mol-1) = 0...
1. 2 KO2(S) + CO2(g) K2CO3(S) + 3/2 O2(g) K = 0.0198 at 315 K AH = -183.6 kJ a. Calculate the value of K at 315 K, for reaction 2: 2. 2 K2CO3(s) + 3 O2(g) 4 KO2(s) + 2 CO2(g) b. Write the K equilibrium expression for reaction 1. c. Calculate the value of Kp for reaction 1 at 315 K.
Using the data: C2H4(g), = +51.9 kJ mol-1, S° = 219.8 J mol-1 K-1 CO2(g), = ‑394 kJ mol-1, S° = 213.6 J mol-1 K-1 H2O(l), = ‑286.0 kJ mol-1, S° = 69.96 J mol-1 K-1 O2(g), = 0.00 kJ mol-1, S° = 205 J mol-1 K-1 calculate the maximum amount of work that can be obtained, at 25.0 °C, from the process: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l)
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for the reaction increases from 93.5 M-1s-1 at 497.7 K to 1349.3 M-1s-1 at 636.7 K. do not include units, but make sure your answer is in kJ/mol! 2) A chemist constructs a plot of ln k vs. 1/T for a chemical reaction. The slope of the trendline for the data is -746 K. What is the activation energy for this reaction in kJ/mol? R...
Find AG (in kJ mol-1 to one decimal place) for the following reaction at 198.15 K when Phi= 2.0 atm, Piz=5.0 atm, and PH2=3.0 atm. H2(g) +12(8) —HI(g)
1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous 2. Consider a...
K2 K →X () На Figure 3: 3. (a) Find T(s) = xtransfer function by reducing the block diagram shown in Figure 3 for K; and H;s. (b) Find the positions of roots of the denominator polynomial of T(s) in s-plane by using Routh table (Routh-Hurwitz criteria) for Ki = , K2 = 1, H2 = 1 and H2 = 3+1 (C) Analyse the stability of the system and explain your findings.
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3 (g) The conditions for this reaction are: PO2 = 1.64 bar PO3 = 1.28 bar .