The rate constant for the decomposition of hydrogen iodide (HI) at 700C equals 0.00160 M-1.s-1: 2HI(g)...

 

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The rate constant for the decomposition of hydrogen iodide (HI) at 700°C equals 0.00160 M-1.s-1: 2HI(g) H2(g) + l2(g) 1 Based on the units of the rate constant, is the reaction first order or second order? Explain. 2 Suppose a reaction is started with 0.0552 mol of HI in a volume of 735 cm³. How many minutes will the reaction take for the moles of HI to drop by 66.6%? 3 Calculate the moles of HI that will remain after 15 minute and 25 seconds. 4 Calculate the half-life (in minutes) for the reaction. The rate constant for the decomposition of hydrogen iodide (HI) at 700°C equals 0.00160 M-1.s-1: 2HI(g) H2(g) + l2(g) 1 Based on the units of the rate constant, is the reaction first order or second order? Explain. 2 Suppose a reaction is started with 0.0552 mol of HI in a volume of 735 cm³. How many minutes will the reaction take for the moles of HI to drop by 66.6%? 3 Calculate the moles of HI that will remain after 15 minute and 25 seconds. 4 Calculate the half-life (in minutes) for the reaction.