Author Question: Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine ... (Read 101 times)

asan beg · **on:** Nov 18, 2019

Question 1

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation:

2NO2(g) → 2NO(g) + O2(g).

A sample of NO2(g) is initially placed in a 2.50 L reaction vessel at 300 °C. If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol-1 s-1, respectively, how many moles of NO2 were in the original sample?
◦ 0.17 mol
◦ 5.9 mol
◦ 15 mol
◦ 0.42 mol

Question 2

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation:

2HI(g) → H2(g) + I2(g)

At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 mol L-1 to 3.50 × 10-2 mol L-1. What is the rate constant for the reaction at this temperature?
◦ 9.69 × 10-2 L mol-1 s-1
◦ 1.95 × 103 L mol-1 s-1
◦ 10.3 L mol-1 s-1
◦ 5.12 × 10-4 L mol-1 s-1

bpool94 · **Reply #1 on:** Nov 18, 2019

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