AP Chem studying
Consider the first order decomposition of hydrogen peroxide: If the half-life for this reaction is 11 hours, how many hours will it take for the concentration to fall to 12.5% of its original value?
C) 33 hours (half-life equation)
The proposed elementary steps of a reaction are shown below. What would be the products of the overall reaction? (Has Ce, Mn and Ti)
B) Ce3+ and Ti3+
In the mechanism given in question (#) what is the catalyst?
B) Mn2+ (catalysts show up in reactants in first step and come back in products of last step)
2N2O5 > 4NO2 + O2 A sample of N2O5 was placed in an evacuated container, and teh reaction represented above occurred. The value of P.N2O5, the partial pressure of N2O5, was measured during the reaction recorded in the table below.
B) The decomposition of N2O5 is a first-order reaction (It's the R^2 closest to 1. P.N2O5 is zeroth, ln(P.N2O5) is first, 1/P.N2O5 is second)
Magnesium reacts with hydrochloric acid to produce hydrogen gas. An experiment was set up to determine the rate of production of the hydrogen gas by measuring its change in volume over the first 60 seconds of the reaction. Magnesium ribbon was cut into squares of .5 cm^2 and 1 cm^2. The volume of hydrochloric acid solution and the total mass of magnesium were held constant in each trial. Which set of conditions would produce the highest rate of production of hydrogen gas?
(D) 3 M HCl, 0.5 cm^2 pieces of magnesium
A kinetics experiment is set up by batman to collect the gas that is generated when a sample of chalk, consisting primarily of CaCO3, is added to a solution of ethanoic acid, CH2COOH. The rate of reaction between CaCO3 and CH3COOH is determined by measuring the volume of gas generated at 25'C and 1 atm as a function of time. Which of the following is most likely to increase the rate of gas production?
D) Decreasing the particle size of CaCO3 by grinding it into fine powder
Consider the following mechanism for the reaction represented above: Step 1: 2NO > N2O2 (fast) Step 2: N2O2 + O2 > 2NO2 (slow)
D) the rate law that is consistent with the mechanism is rate k=[NO]2 [O2]