4)
m(water) = 50.0 g
T(water) = 25.7 oC
C(water) = 4.184 J/goC
m(copper) = 2.55 g
T(copper) = 89.5 oC
C(copper) = 0.385 J/goC
T = to be calculated
Let the final temperature be T oC
use:
heat lost by copper = heat gained by water
m(copper)*C(copper)*(T(copper)-T) = m(water)*C(water)*(T-T(water))
2.55*0.385*(89.5-T) = 50.0*4.184*(T-25.7)
0.9817*(89.5-T) = 209.2*(T-25.7)
87.8666 - 0.9817*T = 209.2*T - 5376.44
T= 25.998 oC
Answer: 26.0 oC
4. Suppose a hot (89.5°C) piece of copper metal (c = 0.385 g K-') with a...
A 83.0 g piece of metal with specific heat 0.622 Jg∘C and at 107∘C is placed in 300. g of water at 26.0∘C. What will be the final temperature of the water? Use 4.184Jg∘C for the specific heat of water.
Copper metal has a specific heat of 0.385 J/g·°C. Calculate the amount of heat required to raise the temperature of 22.8 g of Cu from 20.0°C to 875°C.
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6Q11
A 446-g piece of copper tubing is heated to 89.5 degree C and placed in an insulated vessel containing 159 g of water at 22.8 degree C. Assuming no loss of water and a heat capacity for the vessel of 10.0 J/degree C, what is the final temperature of the system (c of copper = 0.387 J/g degree C)? degree C
Copper metal has a specific heat of 0.385 J/g·°C. Calculate the amount of heat required to raise the temperature of 22.8 g of Cu from 20.0°C to 875°C. a. 1.0 × 10-2 J b. 1.97 × 10-5 J c. 7.51 kJ d. 329 J e. 10.5 kJ
35. Consider the following specific heats of metals. Metal Specific Heat Copper 0.385 J/(g. °C) Cobalt0.418 J/(g °C) Chromium 0.447 J/(g. °C) Gold Silver0.237 J/(g. °C) 0.129 J/(g.°C) If the same amount of heat is added to 100-g samples of each of the metals, which are all at the same temperature, which metal will reach the lowest temperature? a. copper b. cobalt c chromium d. gold e. silver x 36. The sign of AH for the process 12(s)- 12(3) is...
If 400 J of heat were added to 100 g copper (specific heat = 0.385 J/g°C) and 400 J were added to 100 g of gold (specific heat = 0.129 J/g°C), which metal, copper or gold, would have the lower final temperature?
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