please someone help me with question 2. thank you 2. For a second-order reaction where Alaal...
Hello! Can someone help me with this question? Thank you! 6 Consider the following equilibrium at 200 °C in an 80.0 L vessel. 2 NO2 (8) H 2NO(g) + O2(g) At equilibrium, there are 1.88 mol of NO2, 0.120 mol NO, and 0.0600 mol O2 in the reaction vessel Calculate Kc for the reaction at this temperature.
The reaction 2A → B is second order with a rate constant of 51.0/M · min at 24 ° C. (a) Starting with [A]0 = 9.30 ×10−3M, how long will it take for [A]t = 2.80 ×10−3M? min (b) Calculate the half-life of the reaction. min
Be sure to answer all parts. The reaction 2A B is second order with a rate constant of 51.0/M-min at 24°C. (a) Starting with [Alo 8.90 x 10 M, how long will it take for [A],3.30 x 103 M? min (b) Calculate the half-life of the reaction. min
9. The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.50 × 10−3M, how long will it take for [A]t = 3.10 × 10−3M? ______ min (b) Calculate the half-life of the reaction. _______ min 10. The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first-order reaction: 4PH3(g) → P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. a) Calculate...
please help me with both. TIA The following chemical reaction: A → products shows zero order kinetics with respect to A; rate = k[A]º. if k = 9.65 x 10-3 moll's and the initial concentration of A is 0.622 mol L-1, what is the half life of this reaction in minutes? You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104 should be...
[time] [Z] 4. Suppose the data shown are for the second order reaction: → products. What is the value of the rate constant k? O min 50.000 atm 6.250 3.333 2.273. 5. For a first order reaction (G - products) with k = 0.173 min', suppose a chemist runs the reaction starting with an initial concentration [G]. = 12.0 M. a. How many minutes will it take for [G] to decrease to 4.70 M? b. What [G] will remain after...
Could I get help on part B 3a. A certain first-order reaction is 35.5% complete in 4.90 minutes at 25°C. What is its rate constant e-kt K,=0.0895 min 64.5% min - 10 0.645 1.00 to = 8.95 x 100% 4.905 -0.0895 min 3b. If a first-order reaction has an activation energy of 104,600 J/mole and an A value of 5 x 10 sec !, at what temperature will the reaction have a half-life of 1 min? What about 30 days?
Hi! Can someone help me with this question? Thank you! How will the activation energy and the rate constant change if a catalyst is added at 323 K? (c) How will the activation energy and the rate constant change if a catalyst is added at 323 K?
This is the third time I've posted this question. Can someone please help me with the top one. I slipped in a similar example. And the answer is not 2.4135 Consider the following cell reaction Fe(s)2 H ? M)-Fe2(100 M) +H>(g\1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH Consider the following cell reaction Ni(s)2 H (? M) Ni(100 M)Hg100 atm) If the cell potential at 298 K...
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...