The arrhenius equation is
ln(K2/k1) = Ea/R[1/T1 - 1/T2]
K2 = 8.0 L/mole* s, T2 = 360 k
K1 = 4.0 L/mole* s, T1 = 310 k
Ea = x kj/mol , R = 8.314*10^-3 kj.k-1.mol-1
ln((8.0/4.0)) = ((x)/(8.314*10^-3))((1/310)-(1/360)
x = 12.86
Ea = activation energy of the reaction = 12.86 KJ/mol
6. Find the 2nd order reaction's activation energy with the given information. k=4.0L/mol*s at 370 k=8.0L/mol*s...
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if the activation energy for a given compound is found to be 42 kJ/ mol, with a frequency factor of 8.0x10^10 /s, what is the rate constant for this reaction at 298 K?
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Calculate the activation energy, Ea, for N2O5(g) --> 2 NO2(g) + 1/2 O2(g) given k (at 30.0 °C) = 7.24E-5 s–1 and k (at 75.0 °C) = 2.16E-2 s–1. (R = 8.314 J/K×mol)
Given the following reactions, find the lattice energy of KI: K*(g) + F(g) → Kl(s) K(s) → K(g) AH, = 89.6 kJ/mol K(g) → K+(g) + e AHE = 418.9 kJ/mol 1z(s) → 21(g) AH, = 213.6 kJ/mol I(g) +e → (g) AHEA = -295.2 kJ/mol K(s) + 0.5 12(s) → Kl(s) AH, = -328 kJ/mol
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The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1×10−8 s−1. What is the value of the rate constant at 765.0 K? k= s−1
1.) The reaction 2NOCl(g) → 2NO(g) + Cl2 (g) has an activation energy of 100.0 kJ/mol and a rate constant at 350.0 K of 8.5 x 10-6 mol-1 L s-1. Determine the rate constant at 400 K. 2.) For the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) it was found that at a given temperature and after a certain time the rate of formation of H2O(g) was 0.27 mol L-1 s-1. What is the rate of consumption of O2 (g)...
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