A 4.82g sample of iron is heated to 84.3 degrees celsius. A 1.25g sample of gold

Question

A 4.82g sample of iron is heated to 84.3 degrees celsius. A 1.25g sample of gold is heated to 95.1 degrees celsius. Both of these metals are added to 9.47g of cold water that is initially at 14.5 degrees celsius.

a. From the first law of thermodynamics, what is the equation relating the sum of the heats of the two components?

b. Algebraically substitute in the specific heat capacities for the metals and water, the masses of the samples, and the temperature change.

c. Solve the algebraic problem in (b) for Tf, the final temperature of the water.

d. Determine the final temperature of the metals in the water. Hint: its the same for all three components.

Explanation / Answer

heat lost by iron + heat lost by gold + heat gained by water =0

4.82 x specific heat( T - 84.3) + 1.25 x specific heat ( T - 95.1) +
+ mass water x 4.18 ( T - 14.5)=0

find the specific heat of Fe and Au to find the final temperature

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