Chemical Kineti...

The reaction $$A(g)\longrightarrow B(g)+2C(g)$$ is a first order reaction with rate constant $$2.772\times { 10 }^{ -3 }s^{ -1 }$$. Starting with $$0.1$$ mole of $$A$$ in $$2$$ litre vessel, find the concentration of $$A$$ after $$250sec$$ when the reaction is allowed to take place at constant pressure at $$300K$$? (Given ln2= 0.693)

For a given reaction of the first order, it takes 15 minutes for the concentration to drop from 0.8 M to 0.4 M. The time required for the concentration to drop from 0.1 M to 0.025 M will be :

A reaction occurs in parallel paths. For each path having energy of activation as $$E,\ 2E,\ 3E,\ ... nE$$ and rate constant $$K,\ 2K,\ 3K,\ .... nK$$ respectively. If $$E_{AV}=3E$$, then find out the value of $$n$$.

The decomposition of $$Cl_2O_7$$ at 400 K in gaseous phase to $$Cl_2$$ and $$O_2$$ is 1st order reaction. After 55 sec at 400 K, the pressure of reaction mixture increases from 0.62 to 1.88 atm. Calculate the rate constant of the reaction. Also, calculate the pressure of reaction mixture after 100 seconds:

A compound $$A$$ dissociate by two parallel first order paths at certain temperature
$$A(g)\xrightarrow [  ]{ { k }_{ 1 }({ min }^{ -1 }) }  2B(g)$$  $${ k }_{ 1 }=6.93\times { 10 }^{ -3 }min^{ -1 }$$
$$A(g)\xrightarrow [  ]{ { k }_{ 2 }({ min }^{ -1 }) }  C(g)$$  $${ k }_{ 2 }=6.93\times { 10 }^{ -3 }min^{ -1 }$$
The reaction started with $$1$$ mole of pure '$$A$$' in $$1$$ litre closed container with initial pressure $$2$$ atm. What is the pressure (in atm) developed in container after $$50$$ minutes from start of experiment?

The reaction  $$cis-X\overset { { k }_{ f } }{ \underset { { k }_{ b } }{ \rightleftharpoons  }  }  tran-X$$ is first order in both directions. At $${ 25 }^{ o }C$$, the equilibrium constant is $$0.10$$ and the rate constant $$ { k }_{ f }=3\times { 10 }^{ -4 }s^{ -1 }$$. In an experiment starting with the pure $$cis-$$form, how long would it take for half of the equilibrium amount of the $$trans-$$ isomer to be formed?

Mathematical expression for $$t_{1/4}$$ i.e., when $$(1/4)^{th}$$ reaction is over following first order kinetics can be given by:

In the thermal decomposition of $$N_2O$$ at 830 K, the time required to decompose half of the reactant was 263 sec at the initial pressure 290 mm. It takes 212 sec to decompose half of the reactant if initial pressure was 360 mm. What is the order of the reaction? Also calculate $$t_{1/2}$$ for $$N_2O$$ decomposition if initial pressure of $$N_2O$$ is 1 atm.