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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)`
A reaction follows the given concentration-time graph. The rate for this reaction at `20 s` will be

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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) 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) 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

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

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: