I need help with this problem.
A 54.43 gram sample of aluminum (0.900 j/g deg. c) at 25.6 c is heated to 71.4 deg. c. How much energy in calories did the sample gain (1 cal = 4.184 j)? (report answers to the proper number of significant figures)
q in joules = mass x specific heat x (Tfinal-Tinitial)
q in joules = 54.43 x 0.900 J/g*C x (71.4-25)
Solve for q in joules and convert to calories.
cal = joules from above x 1 cal/4.184 J
Post your work if you get stuck.
Thank you!
I got 2243.6046 q and converted that into calories and got 536.234369025 cal. Now I don't know what the proper number of significant figures would be for my final answer.