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You would like to determine the reaction enthalpy for Zn(s) + 2HCl(aq) ? ZnCl2(aq) + H2(g) In part 1 of your experiment you mix 50.0 ml of 2.00 M HCl with 50.0 ml of 2.00 M NaOH. Temperature of the solution rises from 16.9 to 30.4 oC. You determine the density of the resulting solution to be 1.04 g/ml. In part 2 of your experiment you use 100.0 ml of 1.0 M HCL and 1.3078 g of Zn(s). Density of 1.0 M HCl is 1.015 g/ml and heat capacity of the ZnCl2 solution is 3.95 J g-1 K-1. In addition, you look up the heat capacity of water (4.18 J g-1 K-1) and 1.0 M NaCl (3.93 J g-1 K-1); the enthalpy of neutralization for NaOH and HCl is -57.32 kJ mol-1. a) determine calorimeter constant b) determine reaction enthalpy for the Zn / HCl reaction c) if ?fHo (ZnCl2 aq) is -482.2 kJ mol-1 and ?fHo (HCl aq) is -165.2 kJ mol-1, what is you percent error?
Show all the steps in the mechanism for the following reaction, When benzene is mixed with deuterated sulfuric acid, deuterium is slowly incorporated onto the ring. Show the mechanism for this reaction and explain how this relates the sulfonation of ..
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