University of Guelph

In the titration of 80.0 mL of 0.150 M ethylamine, C2H5NH2, with 0.100 M HCl, find the pH at each of the following points in the titration. a. Initially, before any HCl has been added. b. At the halfway point in the titration. c. At the endpoint. d. At 1/4 completion (the "one fourth of the way point") e. At 3/4 completion f. 10.0 mL of HCl beyond the endpoint.

The activation energy for the reaction N2O(g) → N2(g) + O(g) is 250 kJ/mol. If the rate constant is 3.4 s–1 at 1050 K, at what temperature will the rate constant be one thousand times smaller? answer is 846K Use the "all in one equation" to solve for the second temperature: ln{k2/k1} = Ea/R {(1/T1) - (1/T2)} to show how you solved it

A first order reaction is 38.5% complete in 480 seconds. How long will it take for the reaction to go to 95% completion? Question 20 options: 1200 seconds 26 seconds 3000 seconds 600 seconds 480 seconds

What is the logarithm of the equilibrium constant, log K, at 25°C of the voltaic cell constructed from the following two half-reactions? mc077-1.jpgmc077-2.jpgmc077-3.jpg Ag+(aq) + e–mc077-4.jpgAg(s); E° = 0.80 V Question 3 options: 13.5 40.6 6.7 20.3 67.6

The activation energy for the reaction N2O(g) → N2(g) + O(g) is 250 kJ/mol. If the rate constant is 3.4 s–1 at 1050 K, at what temperature will the rate constant be one thousand times smaller?

The balanced chemical equation and rate law for the reaction between NO(g) and H2(g) at a particular temperature are 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) Rate = k[NO]2[H2] What is the reaction order with respect to hydrogen?