Chemical Kineti...

The total pressure of the vessel after $$75$$ minute, if the volume of liquid $$S$$ is supposed to be negligible is:

The decomposition of $$ {\mathrm{N}_{2}}\mathrm{O}_{5} $$ according to the equation $${\mathrm{2N}_{2}}\mathrm{O}_{5}(g)\rightarrow \mathrm{4 NO}_{2}+O_{2}(g) $$ is a first-order reaction. After 30 min from the start of decomposition in a closed vessel the total pressure developed is found to be 284.5 mm Hg. On complete decomposition, the total pressure is 584.5 mm Hg. The rate constant of the reaction is :

The reaction is given below, the rate constant for disappearance of A is $$7.48\times10^{-3}sec^{-1}$$. The time required for the total pressure in a system containing A at an initial pressure of 0.1 atm to rise to 0.145 atm is:
$$2A(g)\rightarrow 4B(g)+C(g)$$

The reaction $$A(aq) \rightarrow B(aq)+C(aq)$$ is monitored by measuring optical rotation of reaction mixture at different time interval. The species A, B and C are optically active with specific rotations $$20^{\circ}, 30^{\circ}$$ and $$-40^{\circ} $$ respectively. Starting with pure A if the value of optical rotation was found to be $$2.5^{\circ}$$ after $$6.93^{\circ}$$ minutes and optical rotation was $$-5^{\circ}$$ after infinite time. Find the rate constant for the first-order conversion into A into B and C:

$$A(aq)\longrightarrow B(aq)+C(aq)$$ is a first order reaction.

Time	$$t$$	$$\infty$$
moles of reagent	$${ n }_{ 1 }$$	$${ n }_{ 2 }$$

Reaction progress is measure with help of titration '$$R$$'. If all $$A,B$$ and $$C$$ reacted with reagent and have '$$n$$' factors [$$n$$ factor; $$eq.wt=\cfrac {mol.wt.}{n}$$] in the ratio of $$1:2:3$$ with the reagent. The $$k$$ in terms of $$t,{ n }_{ 1 }$$ and $${ n }_{ 2 }$$ is :

Two first order reaction have half-lives in the ratio $$8:1$$. Calculate the ratio of time intervals $${ t }_{ 1 }$$ and $${ t }_{ 2 }$$ are the time period for the $${ \left( \cfrac { 1 }{ 4 }  \right)  }^{ th }$$ and $${ \left( \cfrac { 3 }{ 4 }  \right)  }^{ th }$$ completion.

Assertion: In a reversible endothermic reaction, $$E_{act}$$ of forward reaction is higher than that of backward reaction.

The gaseous decomposition reaction, $$A(g)\longrightarrow 2B(g)+C(g)$$ is observed to first order the excess of liquid water at $${ 25 }^{ o }C$$. It is found that after $$10$$ minutes the total pressure of system is $$188$$ torr and after very long time it is $$388$$ torr. The rate constant of the reaction (in $$hr^{ -1 }$$) is:
[Given: vapour pressure of $${ H }_{ 2 }O$$ at $${ 25 }^{ o }C$$ is $$28$$ torr. ($$\ln { 2 } =0.7,\ln { 3 } =1.1,\ln { 10 } =2.3$$)]

For a first-order homogeneous gaseous reaction, $$A\longrightarrow 2B+C$$.
If the total pressure after time $$t$$ was $${ P }_{ t }$$ and after long time $$(t\rightarrow \infty )$$ was $${ P }_{ \infty }$$ then $$k$$ in terms of $${ P }_{ t },{ P }_{ \infty }$$ and $$t$$ is :