In a first-order reaction at 300 K, the half-life is 2.50 x 104 seconds and the...
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In a first-order reaction at 300 K, the half-life is 2.50 x 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 350 K?
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4.78 s-1
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2.79 x 10-5 s-1
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6.38 x 1016 s-1
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7.47 x 10-8 s-1
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1.03 x 10-2 s-1
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Homework Answers
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In a first-order reaction at 300 K, the half-life is 2.50 x 104
seconds and the...
A first order reaction has 2.81 s half-life at 298 K and 0.313 s half-life at...
A first order reaction has 2.81 s half-life at 298 K and 0.313 s half-life at 318 K. Using the Arrhenius expression, identify the correct activation energy for this reaction? (R = 0.00832 kJ/mol-K) O 1. 10.5 kJ/mol 2.86.3 kJ/mol 3. 105 kJ/mol 4.501 kJ/mol
The half-life for the reaction below was determined to be 2.14 x 104 s at 800...
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 226.00 kJ/mol N20(g)N2(8) +0(g) 4th attempt See Periodic Table See Hint What would be the half-life at 1050.43 K? 33.3
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life...
The half-life for the reaction was determined to be 2.14 × 104 s at 800 K....
The half-life for the reaction was determined to be 2.14 × 104 s at 800 K. The value of the half-life is independent of the inital concentration of N2O present. The activation energy of the reaction is 259.00 kJ/mol. N2O(g)->N2(g)+O(g) what would be the half life at 900.10K?
A first order reaction has a half-life of 196 seconds at 25oC. How long (in minutes)...
A first order reaction has a half-life of 196 seconds at 25oC. How long (in minutes) does it take for the concentration of the reactant to drop to 3.125% of the original concentration? (it's not 16.34) The rate constant of a chemical reaction increased from 0.197 s-1 to 3.24 s-1 after raising the temperature from 20.0 oC to 60.0 oC. What is the activation energy (in kJ/mol) for this reaction? (Hint: Think about what R value to use and what...
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and...
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and the activation energy is 64 kJ/mol. What is the rate constant at 20°C? (R-8.314 J/mol x K) 0 a. 6x 10451 b.4.3 x 1045-1 OC. 4.1 x 10851 Od. 1.2 x 10051 Oe-2.2 x 1045-1
The half-life for the reaction below was determined to be 2.14 x 10's at 800 K....
The half-life for the reaction below was determined to be 2.14 x 10's at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 259.00 kJ/mol. NO(g) - Nag) +0g) 1st attempt See Periodic Table See Hint What would be the half-life at 1000.32 K?
Half-life equation for first-order reactions: t1/2=0.693k where t1/2 is the half-life in seconds (s), and k...
Half-life equation for first-order reactions: t1/2=0.693k where t1/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s−1). a) What is the half-life of a first-order reaction with a rate constant of 4.80×10−4 s−1? b) What is the rate constant of a first-order reaction that takes 188 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. c)A certain first-order reaction has a rate constant...
Question 28 For the reaction: 2Ad -- 4 d l the rate law is har et...
Question 28 For the reaction: 2Ad -- 4 d l the rate law is har et = K[A] Atence of 190Khan is 517 Kl/mol and the half-life is 125 10 seconds. Determine the rate constant 300K 5510-14-1 5.6 10' O2710 7.2910 5610 Question 28 For the reaction: 2 A(g) + 4B(g) + C(g) the rate law is: At = [a] At kJ/mol and the half-life is 1.25 x 104 seconds. Determine the rate constant at 300 K? 1 pts At...
The rate constant for this second-order reaction is 0.430 M-'.s at 300 °C. A- products How...
The rate constant for this second-order reaction is 0.430 M-'.s at 300 °C. A- products How long, in seconds, would it take for the concentration of A to decrease from 0.670 M to 0.310 M? 1 = 6.355 Incorrect Calculate the rate constant, k, for a reaction at 56,0 °C that has an activation energy of 88.6 kJ/mol and a frequency factor of 6.85 x 10's-1 k= 2.2188 SI Incorrect
d listing r. (Individ For a particular first-order reaction, it takes 24 minutes for the concentration...
d listing r. (Individ For a particular first-order reaction, it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value, what is the value for rate constant (in S-1) for the reaction? A) 2.0-104 s-1 B)9.6 x 10-4 s-1 C) 1.2 × 10-2 s-1 D)5.8 102s-1 12. In the first order reaction A → products, [A1-0.400 M initially and 0250 M after 15.0 mun, what willl after 175 min? e A) 1.67-10-3 M...
A first order reaction has 2.81 s half-life at 298 K and 0.313 s half-life at 318 K. Using the Arrhenius expression, identify the correct activation energy for this reaction? (R = 0.00832 kJ/mol-K) O 1. 10.5 kJ/mol 2.86.3 kJ/mol 3. 105 kJ/mol 4.501 kJ/mol
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 226.00 kJ/mol N20(g)N2(8) +0(g) 4th attempt See Periodic Table See Hint What would be the half-life at 1050.43 K? 33.3
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life...
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and the activation energy is 64 kJ/mol. What is the rate constant at 20°C? (R-8.314 J/mol x K) 0 a. 6x 10451 b.4.3 x 1045-1 OC. 4.1 x 10851 Od. 1.2 x 10051 Oe-2.2 x 1045-1
The half-life for the reaction below was determined to be 2.14 x 10's at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 259.00 kJ/mol. NO(g) - Nag) +0g) 1st attempt See Periodic Table See Hint What would be the half-life at 1000.32 K?
Question 28 For the reaction: 2Ad -- 4 d l the rate law is har et = K[A] Atence of 190Khan is 517 Kl/mol and the half-life is 125 10 seconds. Determine the rate constant 300K 5510-14-1 5.6 10' O2710 7.2910 5610 Question 28 For the reaction: 2 A(g) + 4B(g) + C(g) the rate law is: At = [a] At kJ/mol and the half-life is 1.25 x 104 seconds. Determine the rate constant at 300 K? 1 pts At...
The rate constant for this second-order reaction is 0.430 M-'.s at 300 °C. A- products How long, in seconds, would it take for the concentration of A to decrease from 0.670 M to 0.310 M? 1 = 6.355 Incorrect Calculate the rate constant, k, for a reaction at 56,0 °C that has an activation energy of 88.6 kJ/mol and a frequency factor of 6.85 x 10's-1 k= 2.2188 SI Incorrect
d listing r. (Individ For a particular first-order reaction, it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value, what is the value for rate constant (in S-1) for the reaction? A) 2.0-104 s-1 B)9.6 x 10-4 s-1 C) 1.2 × 10-2 s-1 D)5.8 102s-1 12. In the first order reaction A → products, [A1-0.400 M initially and 0250 M after 15.0 mun, what willl after 175 min? e A) 1.67-10-3 M...
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