<p>First Year Chemistry</p><p>Worksheet for Rates of Reaction Unit</p><p>For problems 1-5 find the rate law for the reaction using the concentration/rate data. Determine the value of the rate constant along with the units.</p><p>1. H2O2 + 2HI---> 2H2O + I2</p><p>Trial [H2O2] [HI] rate (mol/L/sec) 1 0.10 M 0.10 M 0.0076 2 0.10 M 0.20 M 0.0152 3 0.20 M 0.10 M 0.0152</p><p>2. H2 + I2 ---> 2HI</p><p>Trial [H2] [I2] rate (mol/L/sec) 1 1.0 mol/L 1.0 mol/L 0.20 2 1.0 2.0 0.40 3 2.0 2.0 0.80</p><p>3. 2NO2 + F2 ---> 2NO2F</p><p>Trial [NO2] [F2] rate (mol/L/min) 1 1.0 mol/L 1.0 mol/L 1.0 x 10-4 2 2.0 1.0 2.0 x 10-4 3 1.0 2.0 2.0 x 10-4</p><p>4. 2NO + Br2 ---> 2NOBr</p><p>Trial [NO] [Br2] rate (mol/L/hr) 1 1.0 mol/L 1.0 mol/L 1.30 x 10-3 2 2.0 1.0 5.20 x 10-3 3 4.0 2.0 4.16 x 10-2</p><p>5. ClO3- + 9I- + 6H+ ---> 3I3- + Cl- + 2H2O</p><p>Trial [ClO3-] [I-] [H+] rate 1 0.10 M 0.10 M 0.10 M X 2 0.10 0.20 0.10 2X 3 0.20 0.20 0.10 4X 4 0.20 0.20 0.20 16X</p><p>Given the rate law provided, predict the effect on the initial rate of the following changes in the conditions (temperature, concentration, volume)</p><p>6. Nitrogen monoxide gas and hydrogen gas react according to the rate law Rate = k[NO]2[H2]. How does the rate change if: 1. the concentration of hydrogen is doubled. 2. the concentration of nitrogen monoxide is doubled. 3. the concentration of hydrogen is cut in half. 4. the volume of the container is cut in half. 5. the volume of the container is doubled. 6. the temperature is increased. 7. the concentration of nitrogen monoxide is doubled while the concentration of hydrogen is cut in half. 8. the concentration of hydrogen is doubled while the concentration of nitrogen monoxide is cut in half.</p><p>7. The rate law of a particular reaction between gases X, Y and Z is found to be Rate = k[X]0[Y]2[Z]. How does the initial rate change if:</p><p>1. the concentration of X is doubled. 2. the concentration of Y is tripled. 3. the concentration of Z is quadrupled. 4. the volume of the container is cut in half. 5. the volume of the container is doubled. 6. the temperature is increased. 7. the concentration of X is quadrupled while the concentration of Y and Z are doubled. 8. the concentration of Z is cut in half while the concentration of Y is doubled. 9. the concentration of Y and Z are tripled while the concentration of X is cut in thirds.</p><p>Mechanisms:</p><p>8. Determine the rate laws for the following single-step reactions:</p><p>1. 2NO2 ---> NO + NO3 2. NO3 + CO ---> CO2 + NO2 3. xA + yB ---> zC</p><p>9. For the reactions below, the mechanism is shown. From the mechanism, determine the rate law.</p><p>For the reaction: 2NO2Cl ---> 2NO2 + Cl2 the following mechanism has been proposed:</p><p>STEP 1: NO2Cl --->NO2 + Cl slow STEP 2: NO2Cl + Cl ---> NO2 + Cl2 fast</p><p>Which step is the rate determining step? Explain your reasoning.</p><p>From your choice, write the rate law for the reaction.</p><p>10. The reaction 2NO + O2 ---> 2NO2 exhibits the rate law Rate = k[NO]2[O2]. Which of the following mechanisms is consistent with this rate law? Explain your reasoning.</p><p>1) NO + O2 ---> NO2 + O (slow) O + NO ---> NO2 (fast) 2) NO + O2 ---> NO3 (fast) NO + NO3 ---> 2NO2 (slow)</p><p>3) 2NO ---> 2N2O2 (slow) N2O2 + O2---> N2O4 (fast) N2O4 ---> 2NO2 (fast)</p><p>CHECK YOUR ANSWERS</p><p>Return to Unit</p>