How much energy must be removed from a 200g block of ice to cool it from 0C to -30C?
What is the equation for this?
Q = M*C*(delta T), where
Q is the heat removal required
M = mass of ice
C = specific heat of solid ice
delta T = temperature change (-30 C in this case).
You will need to look up the specific heat of solid ice.
To calculate the amount of energy that needs to be removed from a substance in order to cool it, we can use the equation:
Q = m * C * ΔT
Where:
Q is the amount of energy (in Joules)
m is the mass of the substance (in grams)
C is the specific heat capacity of the substance (in J/g°C)
ΔT is the change in temperature (in °C)
For ice, the specific heat capacity is 2.09 J/g°C.
In this case, the mass of the ice block is 200g, and the change in temperature is from 0°C to -30°C.
Let's plug in the values into the equation to solve for Q:
Q = 200g * 2.09 J/g°C * (-30°C - 0°C)
Simplifying the equation:
Q = 200g * 2.09 J/g°C * (-30°C)
Q = -12,540 J
Therefore, the amount of energy that must be removed from the 200g block of ice to cool it from 0°C to -30°C is 12,540 Joules.
To determine the amount of energy that needs to be removed from the ice, we can use the equation for heat transfer:
Q = m * c * ΔT
Where:
Q is the heat transferred (in joules)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in J/g°C)
ΔT is the change in temperature (in °C)
In this case, we need to find the energy required to cool the ice from 0°C to -30°C, so ΔT would be -30°C - 0°C = -30°C.
The specific heat capacity of ice is approximately 2.09 J/g°C.
Plugging the values into the equation, we have:
Q = 200g * 2.09 J/g°C * (-30°C - 0°C)
Q = 200g * 2.09 J/g°C * -30°C
Q = -12540 J
Thus, the amount of energy that needs to be removed from the 200g block of ice to cool it from 0°C to -30°C is -12540 Joules. Since heat transfer is defined as removing energy from the substance, the negative sign indicates that energy is being removed.