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PL%20Worksheet%206

# PL%20Worksheet%206 - 16.6 Transition theory 6 Draw the...

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PL Worksheet #6 16.4 Integrated Rate Law 1. The reaction: CaSO 4 + MgCO 3 CaCO 3 + MgSO 4 has a rate constant k = 0.0128 L/mol-s. If there is initially 1.85 M of CaSO 4 , how much will CaSO 4 remain after 76 s? 2. In a zero-order reaction, there is 0.25 M of the reactant initially and 0.055 M of the reactant after 125 seconds. What is the half-life of the reaction? 3. For an alpha decay process, where there is initially 2.505 moles of Seaborgium-264 solve for the rate constant if there are 1.251 moles present after 10.00 seconds? 3b. Write a decay reaction for the alpha decay of Seaborgium-264. 3c. How many moles are formed of the new element in 10.00 seconds, using the information in the above two questions? 16.5 Arrhenius Equation 4. A chemical reaction has a rate constant of k = 0.00551 mol/L-s at a temperature of 25 Celsius. At what temperature would the rate constant be k = 0.0112 mol/L-s if the activation energy is 12.5 kJ/mol. 5. What is the reaction order of the chemical reaction discussed in question 4?

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Unformatted text preview: 16.6 Transition theory 6. Draw the transition state in the following reaction: [note, it may be easier to begin with Lewis structures of each compound] H 2 + CO CH 2 O 7. For the diagram below, indicate where the reactants, the transition state and the products would be located. Also label the activation energy of the diagram and the net change in energy. 8. Does the above diagram represent an endothermic or exothermic reaction? 16.7 Reaction Mechanisms 9. For the chemical reaction: 2 HNO 2 + N 2 O 4 NO + H 2 O Is found to be second order with respect to N 2 O and zero order with respect to HNO 2 . 2 N 2 O N 2 + 2 NO ( slow ) N 2 + HNO 2 N 2 O + HNO ( fast ) HNO + HNO 2 H 2 O + 2 NO ( fast ) Does the slow step suggest a rate law that matches experimental evidence? Is this reaction mechanism plausible? Label the intermediates in this reaction mechanism. Describe how increasing the concentration of HNO 2 would effect the overall reaction rate?...
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