An absent-mined prodessie, Mr Waage, took elements A and B in a reaction vessel at room temperature, to study the reaction`A+ 2B rArr 2C +D.` He took the concentration of B as 1.5 times the concentration of A. After the reaction reached equilbrium, he round that the concentrations of A and D were equal. However, he forgot to calculate `K_(c)` and removed oneof the products from the mixture. Now, can you calculate `K_(c)` for the equilibrium attained in his experiment and help him out ?

An absent-mined prodessie, Mr Waage, took elements A and B in a reacti

1.	An absent-mined prodessie, Mr Waage, took elements A and B in a reaction vessel at room temperature, to study the reaction`A+ 2B rArr 2C +D.` He took the concentration of B as 1.5 times the concentration of A. After the reaction reached equilbrium, he round that the concentrations of A and D were equal. However, he forgot to calculate `K_(c)` and removed oneof the products from the mixture. Now, can you calculate `K_(c)` for the equilibrium attained in his experiment and help him out ?
Answer» `A + 2B hArr 2C +D` Initial concentration a 1.5a 0 0 Equilibrium concentration a-x 1.5a-2x 2x x At equilibrium , the concentration of A and that of D are equal `therefore a-x = x implies a=2x ` or ` x=a//2` `K_(c)=((2x)^(2)x)/((a-x)(15a-2x)^(2))` as a=2x `implies (4x^(2).x)/(x xx (x)^(2))implies K_(c) = 4`

Discussion

No Comment Found

Related InterviewSolutions

Hydrogen peroxide decomposes to water abd oxygen. The uncatalysed reaction has activation energy of 86 KJ/mol. The activation energy value in the presence of acetanilide is 112 KJ/mol and in the presence of `MnO_(2)` it is 49 KJ/mol . What conclusion can you draw from the above observations ?
`K_(c)` changes with change in _______.
The decomposition reaction `N_(2)O to N_(2) + O_(2)` takes place on platinum surface. Here, the rate of reaction is independent of the concentrations of the reactant . However, when this reaction is carried out in the absence of platinum surface, the rate of reaction depends on the concentration of the reactant How do you account for this ?
If `K_(C)` for the formatiion of ammonia is 2 `mol^(-2) L^(2)`, `K_(c)` for decoposition of ammonia is ________.
The equilibrium constant for the given reaction, ` CaCO_(3(g)) rarr CaO_(s) +CO_(2(g)) ` is given by :A. `K_(c)=([CaO]*[CO_(2)])/([CaCo_(3)])`B. `K_(c)=([CaO])/([CaCO_(3)])`C. `K_(c)=[CO_(2)]`D. `K_(c)=([CaO])/([CO_(2)])`
Which of the following `k_(c)` values corresponds to the maximum yield of the product ?A. `9.2 xx 10^(2)`B. `1.8 xx 10^(-15)`C. `2.8 xx 10^(3)`D. `3.4 xx 10^(-25)`
A 1 L reaction vessel contained 1 mole each of solid `NH_(4)HS, NH_(30 and H_(2)S` at a temperature of `150^(@)C` . When the decomposition of `NH_(4)HS` was carried out , equilibrium is established `K_(p)` value at that temperature is 100. Calculate the equilibrium partial pressures at which 60 per cent dissociation of `NH_(4)HS` takes place at a lower temperature where `K_(p)` value is equal to 200 `"atm"^(2)` .
Assuming that `2NO + O_(2) to 2NO_(2)` is a single-step reaction, what will be the rate of reaction when the volume of the reaction vessel is reduced of `1//4^(th)` of the initial value ? The original rate of reaction is 64 mol/L/s.
Identify the common property for a chemical reaction at dynamic equilibriumA. The measurable properties like concentration , density , colour, pressure , etc. , remain constant at constant temperature .B. The forward and backward reactions take place with the same rate.C. It can be achieved from both directionsD. all of the above
`2SO_(2(g)) + O_(2(g)) hArr 2SO_(3(g)) + Q ` KJ In the above reaction, how can the yield of product be increased without increasing the pressure ?A. by increasing temperatureB. by decreasing temperatureC. by increasing th volume of the reaction vesselD. by the addition of the catalyst

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment