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For the reaction: aA + bB rarr cC+dD R...

For the reaction: `aA + bB rarr cC+dD`
Rate `= (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt)`
For reaction `3BrO^(ɵ) rarr BrO_(3)^(ɵ) + 2Br^(ɵ)`, the value of rate constant at `80^(@)C` in the rate law for `-(d[BrO^(ɵ)])/(dt)` was found to be `0.054 L mol^(-1)s^(-1)`. The rate constant `(k)` for the reaction in terms of `(d[BrO_(3)^(ɵ)])/(dt)` is

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For the reaction: aA + bB rarr cC+dD Rate = (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt) A reaction follows the given concentration-time graph. The rate for this reaction at 20 s will be

For the reaction: aA + bB rarr cC+dD Rate = (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt) A reaction follows the given concentration-time graph. The rate for this reaction at 20 s will be

For the reaction: aA + bB rarr cC+dD Rate = (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt) The rate of formation of SO_(3) in the following reaction 2SO_(2) + O_(2) rarr 2SO_(3) is 100 g min^(-1) . Hence the rate of disappearance of O_(2) is

For the reaction: aA + bB rarr cC+dD Rate = (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt) The rate of formation of SO_(3) in the following reaction 2SO_(2) + O_(2) rarr 2SO_(3) is 100 g min^(-1) . Hence the rate of disappearance of O_(2) is

For the reaction: aA + bB rarr cC+dD Rate = (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt) In the following reaction, xA rarr yB log.[-(d[A])/(dt)] = log.[(d[B])/(dt)] + 0.3 where negative isgn indicates rate of disappearance of the reactant. Thus, x:y is:

For the reaction: aA + bB rarr cC+dD Rate = (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt) In the following reaction, xA rarr yB log.[-(d[A])/(dt)] = log.[(d[B])/(dt)] + 0.3 where negative isgn indicates rate of disappearance of the reactant. Thus, x:y is:

In the reaction, 3BrO^(-)rarrBrO_(3)^(-)+2Br^(-) (aqueous alkaline medium at 80^(@)C ) the vlaue of the rate constant in the rate law in terms of --(d)/(dt)[BrO^(-)] is 0.056 L "mol"^(-1)s^(-1) . What will be the rate constant when the law is stated in terms of (d)/(dt)[BrO^(-)] ?

The rate of a reaction is expressed in different ways as follows: +(1)/(2)(d[C])/(dt)=-(1)/(2)(d[D])/(dt)=+(1)/(3)(d[A])/(dt)=-(d[B])/(dt) the reaction is