# 2 NOBr (g) - 2NO (g) + Br2 (g) Given the rate is -2.3 mol NOBr L-1hr-1 when the initial concentration was 6.2 M what is the rate constant k? Assume the reaction is 1st order in [NOBr]

Feb 2, 2015

The value of the rate constant $k = 0.37 h {r}^{- 1}$

"NOBrrarr2NO+Br_2

The first order rate expression is:

$- \frac{d \left[N O B r\right]}{\mathrm{dt}} = k \left[N O B r\right]$

$- \left(- 2.3\right) = k \times 6.2$

$k = \frac{2.3}{6.2} = 0.37 h {r}^{- 1}$