Which of the following is not true about "yield"? a. the value of the actual yield must be given in order for the percent yield to be calculated. b. the percent yield is the ratio of the actual yield to the theoretical yield. c. the actual yield may be different from the theoretical yield because reactions do not always go to completion. d. the actual yield may be different from the theoretical yield because insufficient limiting reagent was used.

Explanation:

The choices of a, b, c and d are correct about "yield". For choice d, while insufficient limiting reagent will affect both actual and theoretical yield, it is not an explanation of the difference between actual and theoretical.

So the answer is d.

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 !

it is the most commonly accepted one