One 63-g ice cube at 0.0 °C is dropped into 5.00 × 10² mL of tea to make iced tea. The tea was initially at 20.0 °C. When thermal equilibrium is reached, all of the ice will have melted, and the temperature of the mixture will be somewhere between 20.0 °C and 0.0 °C. Calculate the final temperature of the beverage. Assume the density of the tea is 1.00 g/mL and specific heat capacity is 4.184 J/g. K. The enthalpy of fusion of ice at 0.0 °C is 333 J/g. (Note: The 63 g of water formed when the ice melts must be warmed from 0.0 °C to the final temperature.) Final temperature = °℃

One 63-g ice cube at 0.0 °C is dropped into 5.00 × 10² mL of tea to make iced tea. The tea was initially at 20.0 °C. When thermal equilibrium is reached, all of the ice will have melted, and the temperature of the mixture will be somewhere between 20.0 °C and 0.0 °C. Calculate the final temperature of the beverage. Assume the density of the tea is 1.00 g/mL and specific heat capacity is 4.184 J/g. K. The enthalpy of fusion of ice at 0.0 °C is 333 J/g. (Note: The 63 g of water formed when the ice melts must be warmed from 0.0 °C to the final temperature.) Final temperature = °℃

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)?0.385 J/(g·°C)? Assume no heat is lost to surroundings.
Calculate the energy content (in calories) of a 1.00 g of product that is placed inside a calorimeter having a heat capacity of 950 J/K. Data from the calorimeter indicated that the 3.0 L surrounding water had initial and final temperatures of 18.0 °C and 47.5 °C, respectively. Specific heat capacity of water: 4.18 J/g-K * O 2.6x10^4 cal O 9.5x10^4 cal O 8.8x10^4 cal 7.3x10^4 cal
22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.
Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC). The heat of vaporization for water in the gaseous state is 2260.0 J/g.
A hot lump of 36.1 g of aluminum at an initial temperature of 51.1 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
A sample of cold water was mixed with a sample of hot water inside a calorimeter, and the final temperature of the cold water was 40 °C. Which statement is true about the hot water in the calorimeter? It absorbed 40 joules. It absorbed 80 joules. Its final temperature was 80 °C. or Its final temperature was 40 °C.
Calculate the energy content (in calories) of a 1.00 g of product that is placed inside a calorimeter having a heat capacity of 950 J/K. Data from the calorimeter indicated that the 3.0 L surrounding water had initial and final temperatures of 18.0 °C and 47.5 °C, respectively. Specific heat capacity of water: 4.18 J/g-K a. 2.6x10^4 cal b. 9.5x10^4 cal c. 8.8x10^4 cal d. 7.3x10^4 cal
When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee cup calorimeter, the temperature rises from 21.6 degree C to 37.8 degrees C. The specific heat capacity of water is 4.184 J/(g x degrees C). Calculate the quantity of heat (in kJ) released from the reaction. Assume that the specific heat of the solution is the same as that of pure water.
A 120.0 g sample of a metal at 75.0 °C is added to 150.0 g H20 at 15.0 °C. The temperature of the water rises to 18.3°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. Specific heat capacity for water is 4.18 J / °C g.
A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.