The specific heat of copper metal was determined by putting a piece of the metal weighing 39.4 g in hot water. The quantity of heat absorbed by the metal was calculated to be 47 J from the temperature drop of the water. What was the specific heat of the metal if the temperature of the metal rose 3.10°C?
q = mass x specific heat x delta T
Solve for specific heat. I think Cu has a specific heat of about 0386 J/g*C.
A solution of hydrochloric acid is placed on a balance. Magnesium metal is added and the mass is recorded. The solution is stirred and the mass of the solution is recorded every 10 minutes. The following data is collected:
To find the specific heat of copper metal, we can use the formula:
q = m * c * ΔT
where:
q = quantity of heat absorbed (in joules)
m = mass of the copper metal (in grams)
c = specific heat of copper metal (in J/g°C)
ΔT = change in temperature of the copper metal (in °C)
Given information:
q = 47 J
m = 39.4 g
ΔT = 3.10°C
Now, let's rearrange the formula to solve for the specific heat, c:
c = q / (m * ΔT)
Substituting the given values into the formula:
c = 47 J / (39.4 g * 3.10°C)
First, convert grams to kilograms: 39.4 g = 0.0394 kg
Next, convert the change in temperature to kelvin (since the specific heat is usually given in J/gK): 3.10°C = 3.10 K
Now, let's substitute the values again:
c = 47 J / (0.0394 kg * 3.10 K)
c = 47 J / (0.12194 kgK)
c ≈ 384.7 J/kgK
Therefore, the specific heat of the copper metal is approximately 384.7 J/kgK.