If NaCl is doped with `10^(-3)` mol% of `SrCI_2` what is the concentration of cation vacancies?

If NaCI is doped with 10^(-3) mol % pf SrCl_2 what is the concentration of cation vacancies?

When NaCl is dopped with 10^(-5) " mole % of" SrCl_(2) , what is the no. of cationic vacanies?

Consider a certain reaction A rarr Products with k=2.0 xx 10^(-2) S^(-1) Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L^(-1) .

A solution is saturated in SrCO_(3) and SrF_(2) The CO_(3)^(2-) was found to be 10^(-3) mol/L. If the concentratuonof F^(-) in solution is represented as yxx10^(-2) M then what is the value of y ? ["Given" : K_(sp)(SrCO_(3))=2.5xx10^(-10),K_(sp)(SrF_(2))=10^(-10)]

For an elementary reaction , X(g)toY(g)+Z(g) the half life period is 10 min. In what period of time would the concentration of X be reduced to 10% of original concentration?

Fe(OH)_(2) is diacidic base has K_(b1)=10^(-4) and K_(b2)=2.5xx10^(-6) What is the concentration of Fe(OH)_(2) in 0.1 M Fe(NO_(3))_(2) solution?

The rate constant of the reaction A rarr B is 0.6 xx10^-3 mole per second. If the concentration of A is 5 M, then concentration of B after 20 minutes is:

In the system A_((s))hArr2B_((g))+3C_((g)) , if the concentration of C at equilibrium is increased by a factor of 2 , it will cause the equilibrium concentration of B to change to:

A first order reaction has a rate constant of 0.0051 min^-1 . If we begin with 0.10 M concentration of the reactant, what concentration of reactant will remain in Solution after 3 hours ?

For a first order reaction, k = 2.5xx10^-4 s^-1 , what is the rate of reaction, when the initial concentration of the reactant is 0.1 mol L^-1 ?