Question

A sample of radium-226 decays to form radon-222. A solution of AgNO3 and NaCl reacts to form AgCl and NaNO3. How would an increase in the amounts of reactants affect these reaction rates?

Answer 1

The rate of the chemical reaction increases, but the rate of the nuclear decay stays the same.

Answer 2

Answer: An increase in the amount of radium-226 will increase the reaction rate as radioactive decay follows first order kinetics.

An increase in the amount of  $AgNO_3$ and NaCl will increase the reaction rate as the reaction follows first order kinetics with respect to $AgNO_3$ and first order with respect to NaCl.

$^{226}_{88}\textrm{Ra}\rightarrow^{222}_{86}\textrm{Rn} +^4_2\textrm{He}$

$rate= k[Ra]^1$

If the amount of radium is doubled , the rate of the reaction also doubles.

$AgNO_3 + NaCl\rightarrow AgCl +NaNO_3$

$rate= k[AgNO_3]^1[NaCl]^1$

If only the amount of $AgNO_3$ is doubled , the rate of the reaction also doubles. If only the amount of NaCl is doubled , the rate of the reaction doubles. lf the concentration of  $AgNO_3$ and NaCl both are doubled, the reaction rate becomes 4 times.