For a reaction
`CH_(3)OCH_(3)(g) rarr CH_(4)(g)+H_(2)(g) + CO(g)` at `750 K`,
the rate constant is `6.72 xx 10^(-3) min^(-1)`. Starting with a pressure of `400 mm` of `Hg` at this temperature in a closed container, how many minutes would it take for the pressure in the container to become `760 mm Hg` ?

Explanation

`{:(,CH_(3)OCH_(3)rarr, CH_(4) +, H_(2)+,CO), (t=0,400,0,0,0),(t=t,(400-0),P,P,P):}`
`P_(t) prop 400 - P + P+P+P`
`prop 400 + 2P prop 760`
`2P prop 360`
`P prop 180`
`t = (2.303)/(6.72 xx 10^(-3)) log.(400)/(400-180) = 89.1 min`