135.2 J of heat energy are transferred to 24.75 g of mercury. By how much does the temperature increase? (in K)
Specific heat of the mercury is 140 J/kg·°C.
How much heat is needed to raise the temperature of 24.75 g of water by the same amount?
Specific heat of the water is 4190 J/kg·°C.
Doing something wrong here. help please
dTemp= q/mc= 135.2J/(0.02475Kg*140J/kgC
To determine the temperature increase of mercury, you need to use the formula:
Q = m * c * ΔT
Where:
Q is the heat energy transferred,
m is the mass of the substance,
c is the specific heat of the substance, and
ΔT is the change in temperature.
For the first question, rearrange the formula to solve for ΔT by dividing both sides of the equation by (m * c):
ΔT = Q / (m * c)
Now, plug in the values into the formula:
ΔT = 135.2 J / (24.75 g * 140 J/kg·°C)
First, convert the mass from grams to kilograms by dividing it by 1000:
ΔT = 135.2 J / (0.02475 kg * 140 J/kg·°C)
Now, calculate the change in temperature:
ΔT ≈ 35 °C
Therefore, the temperature of the mercury increases by approximately 35 °C.
For the second question, you can use the same formula and apply it to water. Thus:
ΔT = Q / (m * c)
ΔT = Q / (24.75 g * 4190 J/kg·°C)
Again, convert the mass from grams to kilograms by dividing it by 1000:
ΔT = Q / (0.02475 kg * 4190 J/kg·°C)
Now, calculate the heat energy needed to raise the temperature of water by the same ΔT:
Q = ΔT * (m * c)
Q = 35 °C * (24.75 g * 4190 J/kg·°C)
Again, convert the mass from grams to kilograms:
Q = 35 °C * (0.02475 kg * 4190 J/kg·°C)
Now, calculate the value of Q:
Q = 35 °C * 1.037 J
Q ≈ 36.2 J
Therefore, approximately 36.2 J of heat energy is needed to raise the temperature of 24.75 g of water by the same amount.