Answer:
The specific heat of copper is 0.385 J/g°C
Step-by-step explanation:
A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 425 mL of water at 22.55 degrees Celsius. The final temperature of the water was recorded to be 26.15 degrees Celsius. What is the specific heat of the copper?
Step 1: Data given
Mass of copper = 85.2 grams
Temperature of copper = 221.32 °C
Volume of water = 425 mL
Temperature of water = 22.55 °C
Final temperature = 26.15 °C
Specific heat of water = 4.184 J/g°C
Step 2: Calculat the specific heat of copper
Heat lost = heat gained
Q = m*c*ΔT
Qcopper = -Qwater
m(copper)*c(copper)*ΔT(copper) = - m(water) * c(water) * ΔT(water)
⇒ m(copper) = 85.2 grams
⇒ c(copper) = TO BE DETERMINED
⇒ ΔT(copper) = the change in temeprature = T2 -T1 = 26.15 -221.32 = -195.17 °C
⇒ m(water) = The mass of water = 425 mL * 1g/mL = 425 grams
⇒ c(water) = The specific heat of water = 4.184 J/g°C
⇒ ΔT(water) = The change of temperature of water = 26.15 - 22.55 = 3.6
85.2 * c(copper) * (-195.17) = -425 * 4.184 * 3.6
c(copper) = 0.385 J/g°C
The specific heat of copper is 0.385 J/g°C
(Note, The original question says the volume of the water is 4250 mL. IF this is not an error, the specific heat of copper is 3.85 J/g°C (10x higher than the normal value).