Two 20.0 g ice cubes at -16.0 C are placed into 285 g of water at 25.0 C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.
heat capacity of H2o(s)-->37.7
heat capacity of H2o()-->75.3
enthalpy of fusion of H2o-->6.01
See your post above under Mary.
15 celcius
Sorry! I'm not so sure.
To calculate the final temperature of the water after all the ice melts, we need to determine how much heat is gained or lost by each substance and then apply the principle of conservation of energy.
Here are the steps to solve the problem:
Step 1: Calculate the heat gained or lost by the ice cubes as they melt.
Since the ice is at -16.0°C and there are two ice cubes with a total mass of 20.0 g each, the total heat lost by the ice can be calculated using the formula: q = m × ΔT × C
where q is the heat lost, m is the mass of the ice, ΔT is the change in temperature, and C is the heat capacity.
In this case, ΔT = 0°C - (-16.0°C) = 16.0°C
So, the heat lost by the ice is q = 40.0 g × 16.0°C × 37.7 J/g°C.
Step 2: Calculate the heat gained or lost by the water as it reaches the final temperature.
The final temperature will be the same for both the ice and water, so we can use the same formula for calculating the heat. The initial temperature of the water is 25.0°C.
The mass of the water is 285g, so the heat gained by the water is q = 285g × ΔT × C, where C is the heat capacity of liquid water.
ΔT can be calculated using the formula: ΔT = q / (m × C)
So, the heat gained by the water is q = 285g × ΔT × 75.3 J/g°C.
Step 3: Set up an equation to solve for the final temperature.
The total heat lost by the ice must be equal to the total heat gained by the water. This can be represented as an equation:
q(ice) = q(water)
Step 4: Solve the equation for the final temperature.
Using the equation from step 3, we can substitute the values of q(ice) and q(water) and simplify:
40.0 g × 16.0°C × 37.7 J/g°C = 285 g × ΔT × 75.3 J/g°C
Solving this equation will give us the value of ΔT, which is the change in temperature. The final temperature can be calculated by adding the change in temperature to the initial temperature of the water (25.0°C).
Note: Make sure to convert the units to ensure consistent measurements throughout the calculation.