In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermemeter A chunk of copper weighing 19.97 grams and originally at 97.41 °C is dropped into an insulated cup containing 75.83 grams of water at 23.83 °C. Stiming a The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.52 J/°C. Metal sample Using the accepted value for the specific heat of copper (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings. Tfinal = °C. Submit Answer Retry Entire Group 8 more group attempts remaining

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermemeter A chunk of copper weighing 19.97 grams and originally at 97.41 °C is dropped into an insulated cup containing 75.83 grams of water at 23.83 °C. Stiming a The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.52 J/°C. Metal sample Using the accepted value for the specific heat of copper (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings. Tfinal = °C. Submit Answer Retry Entire Group 8 more group attempts remaining

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...

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In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to Thermometer measure the energy of a solution phase reaction. Stirring rod A student heats 65.13 grams of copper to 98.95 °C and then drops it into a cup containing 84.76 grams of water at 23.02 °C. She measures the final temperature to be 27.86 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.60 J/°C. Water- Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Metal sample Specific Heat (Cu) = J/g°C. 2000 Thomson-BrooksCole
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3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
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A 79.1 g sample of an unknown solid is heated to 62.6ºC and placed into a calorimeter containing 92.1 g of water at 22ºC. If the final temperature of the solid sample and the water is 32.5ºC, what is the specific heat of the solid? Please provide your final answer rounded to two decimal places.
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 38.7 °C. During the reaction 55.6 kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is -1 4.18 J∙g¯¹·K¯¹. Be sure your answer has the correct number of significant digits. 心。 °℃ x10 S
2. A student collect experimental results and show all calculation steps including units. Keep the correet significant figures. Part 1: Calculation of the calorimeter constant (15 pts) Mass of Mass of Temperature of cold water in calorimeter cold water hot water Temperature of hot water before mixing 57.3°C Final temperature of the water after mixing 36.8°C 61.0 g 56.2 g 22.6 °C Show calculations below. Part II: Conduct Reaction 1 between solutions of NaOH and HCI (20 pts) Volume of Volume of Density of the NaOH HCI Initial temperature of the solution in the calorimeter solution solution. solution 51.0 mL 52.0 mL 1.04 g/mL 22.6 °C Show calculations below. Final temperature of the reaction mixture 32.2 °C The calorimeter constant is: Enthalpy of the reaction, in kJ/mol, is
3. Suppose the 25.0 g of the following substances all initially at 27.0 °C absorb 2.35 kJ of energy. What is the final temperature of each? D) Water. You will need to look up specific heat values.
O THERMOCHEMISTRY ARLYQ Using specific heat capacity to find temperature change 0/5 A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 5.80 kg of water at 35.1 °C. During the reaction 67.9 kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J-g answer has the correct number of significant digits. K Be sure your
1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. = 7.52 g = 7.20 g Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water Final temperature of water = 140.0 g = 10.0°C = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.
E Reading list [References) Use the References to access important values if needed for this question. In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 63.30 grams of nickel to 99.15 °C and then drops it into a cup containing 76.81 grams of water at 23.29 °C. She measures the final temperature to be 29.57 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.51 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of nickel. Specific Heat (Ni) J/g°C. Submit Answer Try Another Version 1 item attempt remaining
Together, a pure gold ring and a pure titanium ring have a mass of 15.07 g. Both rings are heated to 94.90 °C and dropped into 13.0 mL of water at 16.80 °C. The water and the rings reach thermal equilibrium at a temperature of 24.20 °C. The density of water is 0.998 g/mL... The specific heat capacity of water is 4.18, the specific heat capacity of gold is 0.129 and the specific heat capacity of titanium is 0.544 Calculate the mass of each ring. mass of gold ring: mass of titanium ring: 50 60