Question

Temp(K) 350 400 k(rate constant, min-1 0.0390 0.0474 Kc(equlibrium constant) 3.9530 1.6187 R = 2cal /...

Temp(K) 350 400
k(rate constant, min-1 0.0390 0.0474
Kc(equlibrium constant) 3.9530 1.6187

R = 2cal / K mol

1)activation energy

2)reaction heat

3)Equilibrium conversion rate

please..

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Temperature (K) k (s–1) 350    9.3 x 10–6 400 6.9 x 10–4 a. (6 pts)...
Temperature (K) k (s–1) 350    9.3 x 10–6 400 6.9 x 10–4 a. (6 pts) Calculate the activation energy (Ea) of this reaction in kJ/mol. b. (3 pts) What is the overall rate order of this reaction? c. (4 pts) Calculate the half-life (t1/2, in seconds) of this reaction at 350 K.
The conversion of cyclopropane an anesthetic, to propylene has a rate constant k=1.3 *10^-6 s^-1 at...
The conversion of cyclopropane an anesthetic, to propylene has a rate constant k=1.3 *10^-6 s^-1 at 400 Celcius and k=1.1 *10^-5 s^-1 at 430 Celcius. What is the activation energy?What is the value of the frequency factor A for this reaction? What is the rate constant for this reacton at 350 C?
A. The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)<---> CH4(g)...
A. The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)<---> CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.346 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. B. The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g) <---> 2 CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.200 moles of CH4and 0.200 moles of CCl4are introduced into a...
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K. CH4 (g) +...
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K. CH4 (g) + CCl4 (g) <-> 2 CH2Cl2 (g) Calculate the equilibrium concentrations of reactants and product when 0.281 moles of CH4 and 0.281 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] = [CCl4] = [CH2Cl2] =
The activation energy, Ea for a particular reaction is 13.6 kj/mol. If the rate constant at...
The activation energy, Ea for a particular reaction is 13.6 kj/mol. If the rate constant at 754 degrees celsius is 24.5/min at egat temperature in celsius will the rate constant be 12.7/min? r= 8.314j/mol • K
Answer the following based on the reaction. At 313 K, the rate constant for this reaction...
Answer the following based on the reaction. At 313 K, the rate constant for this reaction is 1.09×102 /s and at 564 K the rate constant is 6.62×106 /s. cyclopentane → 1-pentene 1. Determine the activation energy (EA) (in kJ/mol) for this reaction. 2. Determine the pre-exponential factor, A (in /s) for this reaction. 3. Determine the rate constant (in /s) for this reaction at 1218 K.
The rate constant of a first-order reaction is 3.20 × 10−4 s−1 at 350.°C. If the...
The rate constant of a first-order reaction is 3.20 × 10−4 s−1 at 350.°C. If the activation energy is 135 kJ/mol, calculate the temperature at which its rate constant is 9.15 × 10−4 s−1.
By what factor does the rate constant increase when the temperature increases from 200. K to...
By what factor does the rate constant increase when the temperature increases from 200. K to 400. K for a reaction with an activation energy of 845 J/mol?
A reaction has a rate constant of 0.393 at 291 K and 1.41 at 345 K....
A reaction has a rate constant of 0.393 at 291 K and 1.41 at 345 K. Calculate the activation energy of this reaction in kJ/mol.
A reaction has a rate constant of 1.13×10−2 /s at 400. K and 0.688 /s at...
A reaction has a rate constant of 1.13×10−2 /s at 400. K and 0.688 /s at 450. K. Determine the activation barrier for the reaction. What is the value of the rate constant at 425 K?