In a certain experiment the decomposition of hydrogen iodide on finely divided gold is zeroth order with respect to HI.
2HI(g) H2(g) + I2(g)
Rate = -d[HI]/dt = k = 1.80×10-4 mol L-1 s-1
If the experiment has an initial HI concentration of 0.320 mol/L, what is the concentration of HI after 19.0 minutes? = .115 mol/L. total time to decompose = 29.6 minutes.
What is the rate of formation of H2 15.0 minutes after the reaction is initiated?
2HI(g) H2(g) + I2(g)
Rate = -d[HI]/dt = k = 1.80×10-4 mol L-1 s-1
If the experiment has an initial HI concentration of 0.320 mol/L, what is the concentration of HI after 19.0 minutes? = .115 mol/L. total time to decompose = 29.6 minutes.
What is the rate of formation of H2 15.0 minutes after the reaction is initiated?