How many calories would be needed to heat 1.65 kg of gold from 12 degrees C to 25 degrees C?
25C-12C=21.45kg
To calculate the number of calories needed to heat a substance, we can use the formula:
Q = m * c * ΔT
Where:
Q = heat energy (in calories)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in calories/gram °C)
ΔT = change in temperature (in °C)
Since gold has a specific heat capacity of 0.031 calories/gram °C, we can substitute the given values into the formula:
m = 1.65 kg = 1650 grams
c = 0.031 calories/gram °C
ΔT = 25°C - 12°C = 13°C
Now, we can calculate the heat energy:
Q = 1650 g * 0.031 cal/g°C * 13°C = 641.03 calories
Therefore, approximately 641.03 calories would be needed to heat 1.65 kg of gold from 12°C to 25°C.
To calculate the number of calories needed to heat a substance, you can use the specific heat capacity equation:
Q = m * c * ΔT
Where:
Q = heat energy (in calories)
m = mass of the substance (in kg)
c = specific heat capacity of the substance (in cal/g°C)
ΔT = change in temperature (in °C)
First, you need to determine the specific heat capacity of gold. The specific heat capacity of gold is approximately 0.031 cal/g°C.
Next, you can plug in the values into the equation:
m = 1.65 kg
c = 0.031 cal/g°C
ΔT = (25°C - 12°C) = 13°C
Converting the mass of gold from kilograms to grams:
m = 1.65 kg * 1000 g/kg = 1650 g
Now, you can calculate the heat energy (Q):
Q = m * c * ΔT
Q = 1650 g * 0.031 cal/g°C * 13°C
Calculating the result:
Q ≈ 651.45 calories
Therefore, approximately 651.45 calories would be needed to heat 1.65 kg of gold from 12°C to 25°C.