SIG FIG QUESTION: A 12.0 g sample of a metal is heated to 90.0 C. It is then dro

Question

SIG FIG QUESTION:

A 12.0 g sample of a metal is heated to 90.0 C. It is then dropped into 25.0 g of water. The temperature of the water rises from 22.5 to 25.0 C. The specific heat of water is 4.18 Jg1C 1 . Calculated the specific heat of the metal. Express your answer in Jg1C 1 .

I know that the answer is 0.335. My question: Should there be 2 sig figs (0.34) because 25-22.5=2.5? Or is it three sig figs 0.335 because all the original values have 3 sig figs in the beginning.

Thanks for the explanation.

Explanation / Answer

Here, apply the equation -

Q = mc*delta(t)

Q = energy (equal for system)

Now, apply the condition

Quantity of heat loss = Quantitity of heat gain

=> m1*c1*delta(t1) = m2*c2*delta(t2)

=> (12g)c(90-25 degrees) = (25g)(4.18)(25 - 22.5 degrees)

=> c = 0.3349 Jg-1degC-1

Answer in three significant digit = 0.335 Jg-1degC-1

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