Answer:
The answer to your question is C = 0.000333 kcal/g°C
or C = 0.333 cal/g°C
Explanation:
Data
Q = 1.67 kcal
mass = 79.2 g
ΔT = 63.3°C
Formula
Q = mCΔT
Solve for C
C = Q/mΔT
Substitution
C = 1.67/(79.2 x 63.3)
Simplification
C = 1.67 / 5013.4
Result
C = 0.000333 kcal/g°C
or C = 0.333 cal/g°C
Answer:
The specific heat of the unknown metal is 0.333 cal/g°C
Explanation:
Step 1: Data given
1.67 kcal of energy is required
Mass of the metal = 79.2 grams
Temperature rise = 63.3 °C
Step 2: Calculate specific heat of the metal
Q = m*c*ΔT
⇒ with Q = the energy required = 1.67 kcal = 1670 cal
⇒ with m = the mass of the metal = 79.2 grams
⇒ with c = the specific heat of the metal = TO BE DETERMINED
⇒ with ΔT = the temperature rise = 63.3 °C
1670 cal = 79.2 grams * c * 63.3 °C
c = 0.333 cal/g*°C
The specific heat of the unknown metal is 0.333 cal/g°C
