The decomposition of dimethyl ether leads to the formation of CH4,H2 and CO and the reaction rate is given by Rate =k[C H3 O C H3](3/2) The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether i.e., Rate =k(PC H3 O C H3)(3/2) If the pressure is measured in bar and time in minutes, then the unit of rate constants is

Question

The decomposition of dimethyl ether leads to the formation of CH4,H2 and CO and the reaction rate is given by Rate =k[C H3 O C H3](3/2) The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether i.e., Rate =k(PC H3 O C H3)(3/2) If the pressure is measured in bar and time in minutes, then the unit of rate constants is (A) bar1 / 2 min (B) bar3 / 2 min- 1 (C) bar- 1 / 2 min- 1 (D) barmin- 1

Tardigrade Admin · Accepted Answer

As rate=k[C H3 O C H3](3/2) bar/min =k(b a r)(3/2) Unit of k=bar- (1/2) m i n- 1

$ba r^{1/2} min$

$ba r^{3/2} mi n^{- 1}$

$ba r^{- 1/2} mi n^{- 1}$

$ba r mi n^{- 1}$

As $r a t e = k [C H_{3} OC H_{3}]^{\frac{3}{2}}$
bar/min $= k (ba r)^{\frac{3}{2}}$
Unit of $k = ba r^{- \frac{1}{2}} mi n^{- 1}$

bar1/2min

bar3/2min−1

bar−1/2min−1

barmin−1

As rate=k[CH3​OCH3​]23​ bar/min =k(bar)23​ Unit of k=bar−21​min−1

$ba r^{1/2} min$

$ba r^{3/2} mi n^{- 1}$

$ba r^{- 1/2} mi n^{- 1}$

$ba r mi n^{- 1}$

As $r a t e = k [C H_{3} OC H_{3}]^{\frac{3}{2}}$
bar/min $= k (ba r)^{\frac{3}{2}}$
Unit of $k = ba r^{- \frac{1}{2}} mi n^{- 1}$