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Write instantaneous rate expression for: 2N2O5(g) → 4NO2(g) + O2(g)


Instantaneous rate expression can written as 

rinst = -12[N2O5]t =14[NO2]t=[O2]t

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For the reaction A + B → 2C at a given temperature, the rate of disappearance of A is found to be 10-2 moles L–1 sec–1. Calculate (i) rate of disappearance of B and (ii) rate of formation of C.

For  a given reaction 
A + B → 2C
we have given 
 the rate of disappearance of A is  10-2 moles L–1 sec–1

(ii)
 rate of expression can be written as 

-d[A]dt=-d[B]dt

since rate of  disappearance of A is given to be 10-2 moles L–1 sec–1
thus 
rate of  disappearance B 10-2 moles L–1 sec–1


(iii)
d[A]dt= 12d[C]dtas given  d[A]dt= 10-2moles L-1 sec-1thus 10-2moles L-1 sec-1 = 12d[C]dtd[C]dt=2x10-2moles L-1 sec-1
for Ans. (i) 10–2 mol L–1 sec–1   (ii) 2 x 10–2mole L–1 sec–1

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Calculate the half-life of the following first order reaction
C2H4 O2(g) → CH4(g) + CO2(g)
Given the initial partial pressure of C2H4O2(g) is 84 mm and the total pressure at the end of 16 min is 110 mm.

For the first order reaction for the gases phase given by

k= 2.303tlogp1p2where p1 =intial pressurep2 = final pressure

we have give p1 = 84mm
total pressure =110mm
at the time = 16 min

thus applying in above formula

k= 2.30316log84110k= 0.1439 log 0.7636 k= 0.1439 x 0.1171k= 0.01685also half life for the first order is given by t1/2 =0.693kt1/2 =0.6930.01685 = 43.31 min


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The rate constant of a reaction is 3 x 10–2 h–1. What is the order of the reaction?

we have given that 

 3 x 10–2 h–1 
since unit of first order reaction is  s-1

thus it is first order reaction

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What is a zero order reaction?

A reaction in which the rate is independent of the concentration of the reactants.

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