In: Chemistry
Suppose that 24 g of each of the following substances is initially at 29.0 ∘C. What is the final temperature of each substance upon absorbing 2.45 kJ of heat?
silver
gold
aluminum
water
Silver: specific heat= 236 J/kg.ºC
1Kg --------- 236 J
24x10-3Kg ----- x= 5.664 J
In order to increase 1ºC the temperature of the silver we need 5.664J, so, if the silver absorbed 2450J, the temperature increased:
5.664 J ------ 1ºC
2450 J ------- x= 432.6 ºC
Final temperature= 29 + 432.6 = 461.6ºC
Gold: specific heat= 130 J/Kg.ºC
1Kg --------- 130 J
24x10-3Kg ----- x= 3.12 J
In order to increase 1ºC the temperature of gold we need 3.12J, so, if the gold absorbed 2450J, the temperature increased:
3.12 J ------ 1ºC
2450 J ------- x= 785.3 ºC
Final temperature= 29+785.3= 814.3ºC
Aluminum: specific heat= 897 J/Kg.ºC
1Kg --------- 897 J
24x10-3Kg ----- x= 21.528 J
21.528 J ------ 1ºC
2450 J ------- x= 113.8 ºC
Final temperature= 29+ 113.8= 142.8ºC
water: specific heat= 4186 J/Kg.ºC
1Kg --------- 4186 J
24x10-3Kg ----- x= 100.464 J
100.464 J ------ 1ºC
2450 J ------- x= 24.4 ºC
Final temperature= 29+785.3= 53.4ºC