A first order reaction has `k=1.5 xx 10^(-6) s^(-1)` at `200^(@)`C. If the reaction is allowed to run for 10 hours, what percentage of initial concentration would have changed in products?

A first order reaction has k=1.5xx10^-6 s^-1 at 200^@C . If the reaction is allowed to run for 10 hours, what percentage of the initial concentration would have changed into the product ? What is the half life period of the reaction ?

A first order reaction has k=1.5xx10^(-6) per second at 240^(@)C . If the reaction is allowed to run for 10 hours, what percentage of initial concentration would have changed to products ? What is the half-life period of this reaction ?

A 1st order reaction has K value 1.5xx10^(-6) at 200^@C . The reaction is allowed to continue for 10 hours. Calculate the percentage of initial concentration that would have changed in the product and also calculate half life period.

The first order reaction has k=1.5xx10^(-6) per second at 200^(@)C . If the reaction is allowed to ruf for 10 hours at the same temperature, what percentage of the initial concentration would have changed into the product? What is the half life period of this reaction ?

The first order reaction has k=1.5xx10^(-6) per second at 200^(@)C . If the reaction is allowed to ruf for 10 hours at the same temperature, what percentage of the initial concentration would have changed into the product? What is the half life period of this reaction ?

A first order gas reaction has k = 1.5 xx 10^(-6) s^(-1) at 200^(@)C . If the reaction is allowed to run for 10 h , what have changed in the Product? What is the half-life of this reaction?

A first order gas reaction has k = 1.5 xx 10^(-6) s^(-1) at 200^(@)C . If the reaction is allowed to run for 10 h , what have changed in the Product? What is the half-life of this reaction?

The rate constant of a first order reaction is 1.5xx10^(-6)s^(-1) at a specific temperature . What percent of initial concentration of the reactant gets converted into product after 10h?