Answer:
Final temperature of the mixture is 50°C
Explanation:
This is a typical calorimetry problem, where the heat yielded by a compound is immediately won by another.
Water at 90°C raise the temperature of water at 10°
Density of water = 1g/mL
Mass of water = 100 g, because the volume is 100mL
If the two pieces of water are in a calorimeter where heat is not released or gained, the sum of both heats is 0
4.18 J/g°C . 100 g ( T°final - 90°C) + 4.18 J/g°C . 100 g ( T°final - 10°C) = 0
418 J/°C T°final - 37620 J + 418 J/°C T°final - 4180J = 0
836 J/°C T°final - 37620J - 4180J = 0
836 J/°C T°final = 41800J
T°final = 41800J / 836 °C/J = 50°C
Answer:
Final temperature of the mixture is 50°C
Explanation:
This is a typical calorimetry problem, where the heat yielded by a compound is immediately won by another.
Water at 90°C raise the temperature of water at 10°
Density of water = 1g/mL
Mass of water = 100 g, because the volume is 100mL
If the two pieces of water are in a calorimeter where heat is not released or gained, the sum of both heats is 0
4.18 J/g°C . 100 g ( T°final - 90°C) + 4.18 J/g°C . 100 g ( T°final - 10°C) = 0
418 J/°C T°final - 37620 J + 418 J/°C T°final - 4180J = 0
836 J/°C T°final - 37620J - 4180J = 0
836 J/°C T°final = 41800J
T°final = 41800J / 836 °C/J = 50°C
