If all of the ice melts add one more piece of ice so that ice is present in the

If all of the ice melts add one more piece of ice so

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minutes, add an additional piece of ice. If all of the ice melts, add one more piece of ice sothat ice is present in the cup for Step 9. Place the lid on the Styrofoam™ cup and place thethermometer in the lid. Continue to swirl the Styrofoam™ cup for approximately two minutes, or until the temperature reading on the thermometer stabilizes. Record the lowest temperature of the mixture of ice and water in Table 4. Use the plastic fork to quickly remove any unmelted ice from the cup. Carefully pour the cold water from the cup into thegraduated cylinder and record the final volume to the nearest mL.
Results and ConclusionsPost Lab Questions1.Calculate the change in the temperature of the hot water.2.Calculate the heat lost by the hot water. Heat must be expressed in kilojoules (kJ). It can be calculated by using the following equation:3.Calculate the volume of ice melted.4.Calculate the mass of ice melted. Remember that the density of water is 1 g/mL.5.Calculate the molar heat of fusion of ice, i.e. the number of kilojoules of heat per mole ice.6.Calculate the percent error in your determination of the value for the molar heat of fusion of ice. 8.In order to do the calculations, you assumed that all of the heat lost by the hot water was absorbed by the ice causing it to melt. Was this assumption correct? Explain.9.Write and equation for the melting of ice. Include the energy term in kJ on the proper sideof the equation.

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