To find the amount of heat absorbed by the ice cube and resulting water, we can use the equation Q = mcΔT. First, we need to find the heat absorbed during the melting of the ice. Then, we need to find the heat absorbed during the change in temperature of the resulting water. Add the two amounts of heat absorbed to find the total heat absorbed by the ice cube and resulting water.
When a person places an ice cube on a burn, heat is transferred from the person's hand to the ice cube, causing it to melt. To find the amount of heat absorbed by the ice and resulting water, we can use the equation:
Q = mcΔT
Where Q is the heat absorbed, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
First, we need to find the heat absorbed during the melting of the ice. The specific heat capacity of ice is approximately 2.09 J/g°C, and we can assume that the heat absorbed during the phase change is equal to the heat released from the hand. Therefore, the equation becomes:
Q = (mass of ice)(specific heat capacity of ice)(ΔT)
Substituting the given values:
Q = (16.5g)(2.09 J/g°C)(0 - (-12.9)°C)
Solving this equation gives us the amount of heat absorbed by the ice cube. To find the total amount of heat absorbed by the ice and resulting water, we need to add the heat absorbed during the change in temperature of the resulting water. The specific heat capacity of water is approximately 4.18 J/g°C. Using the same equation:
Q = (mass of water)(specific heat capacity of water)(ΔT)
Substituting the given values:
Q = (mass of resulting water)(4.18 J/g°C)(28.7 - 0)°C
Add the two amounts of heat absorbed to find the total heat absorbed by the ice cube and resulting water.