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CHM 230 Study Guide - Midterm Guide: Phenolphthalein, Rate Equation, Reaction Rate Constant

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School
Kansas State University
Department
General Chemistry
Course
CHM 230
Professor
All

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Document Summary

Review guide for chemistry 2 laboratory exam 1. The exam has 25 questions, 2 points each. There are questions from each of the first 6 experiments. Know how temperature, concentration, and surface area impacted the rates of the reactions studied. Review how the factors, temperature, concentration and surface area catalyst impact on the reaction in lab. rates. Know how concentration, temperature impact the activation energy and the rate of a reaction. Review how to write the rate equation of a given reaction. Review the calculations of rate constant of the reactions. Know how to determine the rate of the phenolphthalein-hydroxide reaction. Know how to calculate the order of the reaction with respect to both hydroxide and phenolphthalein from experimental data. Know how to determine the rate order for the reaction. Know how to calculate keq and concentration of unknown from fescn+2 experimental data. Know the factors that impact the equilibrium constant.

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Related Questions

Question 1

CaC03(s) +2HCl(aq) ? CaCl2(aq) + +H20(l)

In the reaction above, the rates of consumption of CaC03 doubled when the concentration of HCI was increased from 0.25 M to 0.50 M. What is the order of the reaction with respect to HCI?

Order [x] (numerical)

Question 2

Concentration, temperature, use of catalyst, surface area of particles, nature of reactants, and pressure are all factors that affect the ________of chemical reactions.Fill the blank space with any of the following words; activity, rate, state, reactants, products.

  1. 1.The experimental rate law of a simple reaction A → B + C is v = k[A]. (a) Determine total order of the reaction. (b) Imagine initial conditions at which the rate equals v0. Calculate the change in the reaction rate that will be observed when the concentration of A will be tripled.

2.Calculate the activation energy for a first-order reaction if its rate constant increases from 10 s–1 to 100 s–1 as the temperature increases from 300 to 330 K.

3.Consider a simple first-order reaction A → B. If you start with solution of 0.1 mol/L A, it takes 20 s to go to a concentration of 0.05 mol/L of A. (a) What is the value of the rate constant for this reaction? (b) Calculate half-life of the reaction.