If 9560 J of energy were absorbed by 500. g of ice at 0.0 °C, what would be the final temperature?
Can someone walk me through setting this up?
Sure! To solve this problem, you can use the heat equation:
Q = m * c * ΔT
Where:
Q is the amount of heat transferred
m is the mass of the substance
c is the specific heat capacity of the substance
ΔT is the change in temperature
In this case, we want to find the final temperature, so we need to rearrange the equation to solve for ΔT:
ΔT = Q / (m * c)
Now let's plug in the values given in the problem and calculate the final temperature.
1. Convert the mass of the ice from grams to kilograms by dividing it by 1000:
m = 500 g / 1000 = 0.5 kg
2. The specific heat capacity of ice is approximately 2.09 J/g°C, or 2090 J/kg°C. So:
c = 2090 J/kg°C
3. Plug in these values along with the given amount of energy absorbed:
Q = 9560 J
m = 0.5 kg
c = 2090 J/kg°C
ΔT = 9560 J / (0.5 kg * 2090 J/kg°C)
Now just calculate this expression to find ΔT, which represents the change in temperature:
ΔT = 9560 J / 1045 J/°C
ΔT ≈ 9.15 °C (rounded to two decimal places)
To find the final temperature, subtract the change in temperature from the initial temperature of 0.0 °C:
Final temperature = 0.0 °C - 9.15 °C
Final temperature ≈ -9.15 °C (rounded to two decimal places)
Therefore, the final temperature of the ice after absorbing 9560 J of energy would be approximately -9.15 °C.
heat to melt the ice=Hf*500=you do it.
Heat left over=heat to heat water= 500*c*(Tf) solve for Tf