Which of the following values would you expect for the ratio of half-lives for a reaction with starting concentrations of 0.05m and 0.01m, t1/2(0.05m) / t1/2 (0.01m), if a reaction is known to be zero order?

The expected ratio of half-lives for a reaction will be 5:1.

Explanation:

Integrated rate law  for zero order kinetics is given as:

= initial concentration

[A]=concentration at time t

k = rate constant

if,

, the equation (1) becomes:

Half life when concentration was 0.05 M=

Half life when concentration was 0.01 M=

Ratio of half-lives will be:

The expected ratio of half-lives for a reaction will be 5:1.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !