Aqa a level chem enthalpy help!!

Error's 1 and 2 are correct possible explanation's however Error 3 is incorrect so only A and B

The student's calculated enthalpy change was less exothermic than the value in data books.
Which of the following errors could have contributed to this result?
A) Error 1; After the final temperature was recorded, the student removed the burner from under
the beaker. The flame burnt for a further 5 minutes before weighing the spirit burner.
B) Error 2: The student recorded the final temperature 5 minutes after removing the burner.
C) Error 3: The student spilt some water on the bench when pouring the water from the measuring cylinder into the beaker.

given the errors described, you should assume that the enthalpy was calculated in two steps:

(1: Q = mcδθ to find the thermal energy (which is then presumably converted to kj)

(2: δh = q/n (where n is the moles of the alcohol burned)

from these equations, it can be deduced that:

(a) δh will have a larger magnitude (size) if the value of n used is small and δh will have a smaller magnitude if the value of n used is large.

(b) δh will have a large magnitude if the value of q is large (this is dependent on both m and δθ, since c is a constant) and δh will have a small magnitude if the value of q is small.

For the first error, assume the values of m and δθ are recorded correctly. How would this error affect the value of n and therefore, how would this affect the magnitude of the enthalpy change? Would this imply the reaction is more/less exothermic than it should be?

Use similar logic for the other two errors and you should hopefully get a correct answer.