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Arrhenius Equation

#### Q. 10) For the reaction: 2N2O5(g) →4NO2(g) +O2(g) the rate law is: Δ[O2] Δt =k[N2O5] At 300 K, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2. What is the rate constant at 310 K?

Solved • Jun 26, 2019

Arrhenius Equation

#### Q. 7) The rate constant, k, for the thermal decomposition of acetaldehyde is 0.10 M-1s-1 at 500 K and 0.30 M-1s-1 at 469 K. What is the value of the energy of activation? CH3CHO (l) →CH4 (g) + CO (g) A) 32.0 kJ/mol B) -70.3 kJ/mol C) 0.693 kJ/mol D) -0.693 kJ/mol E) 70.3 kJ/mol

Solved • Jun 26, 2019

Arrhenius Equation

#### Q. 8) What is the rate constant at 305 K for the reaction: 2N2O5 →2N2O4 +O2, ifk = 3.46 × 10-5 s-1 at 298 K and Ea = 106 kJ/mol? A) 1.2 × 10-5 s-1 B) 9.2 × 10-5 s-1 C) 2.4 × 10-5 s-1 D) 4.8 × 10-5 s-1 E) 6.0 × 10-5 s-1

Solved • Jun 26, 2019

Arrhenius Equation

#### Q. 5) The activation energy for a reaction is 24.5 kJ/mol. The rate constant is 7.7 ×10-2 min-1 at 500 K. At what temperature, in Kelvin, will the rate constant be 1.5 ×10-2 min-1? A) 488 B) 184 C) 248 D) 391 E) 692

Solved • Jun 26, 2019

Arrhenius Equation

#### Q. 4) The activation energy for a reaction is 37.6 kJ/mol. The rate constant for the reaction is 5.4 ×10-3s-1 at 45°C. Calculate the rate constant at 145°C. A) 5.5 ×10-3 B) 8.4 ×10-3 C) 0.16 D) 0.38 E) 0.56

Solved • Jun 26, 2019

Arrhenius Equation

#### Q. 3) The rate constant for a particular reaction is 2.7 ×10-2s-1 at 25°C and 6.2 ×10-2s-1 at 115°C. What is the activation energy for the reaction, in kJ/mol? A) 87 B) 8.9 C) 13 D) 0.0045 E) 0.089

Solved • Jun 26, 2019

Arrhenius Equation

#### Q. 8) If the activation energy for a given compound is found to be 103 kJ/mol, with a frequency factor of 4.0 × 1013 s-1, what is the rate constant for this reaction at 398 K? A) 8.2 s-1 B) 1.7 × 1010 s-1 C) 3.9 × 1010 s-1 D) 1.2 s-1 E) 2.5 × 107 s-1

Solved • Jun 26, 2019