Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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There are two pictures, one is the problem and the other is the values for physical constants.
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- these are 2 different questions please label as 1 and 2arrow_forwardIn 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. Water Thermometer Metal sample 2003 Thomson-Brooks/Cole Stirring rod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 100.00 grams of nickel to 98.10 °C and then drops it into a cup containing 79.36 grams of water at 23.62 °C. She measures the final temperature to be 32.36 °C. Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant. Calorimeter Constant = J/°Carrow_forwardIn 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. Thermometer Stirring rod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 97.63 grams of nickel to 97.98 °C and then drops it into a cup containing 78.82 grams of water at 23.75 °C. She measures the final temperature to be 32.34 °C. Water- Metal sample Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant. Thomndrc Calorimeter Constant = | J/°C.arrow_forward
- Res Classify each function as a path function or a state function. Path function State function Answer Bank distance traveled enthalpy energy work heatarrow_forwardA 139-lb student races up stairs with a vertical height of 5.5 m in 5.5 s to get to a class on the second floor. How much power in watts does the student expend in doing work against gravity?arrow_forwardUse the following data to answer part A: mixing NaOH(s) into plain water released 1541 J of heat mixing NaOH(s) into HCl(aq) released 3498 J of heat mixing NaOH(aq) into HCl(aq) released 2000 J of heat Show that this data either supports or contradicts Hess’s Law and be clear in your explanation by using chemical equations and numerical calculations. Assume that all three parts use the same amount of NaOH and for the two parts using HCl(aq), the same amount of HCl was used as well. Hint: The sign of your values are important.arrow_forward
- Hi I am having trouble answering this question. Thank you.arrow_forwardIn 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. Thermometer Metal sample ©2003 Thomson-Brooks/Co Stirring rod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 93.37 grams of zinc to 98.36 °C and then drops it into a cup containing 81.25 grams of water at 21.46 °C. She measures the final temperature to be 28.84 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = J/°Carrow_forward
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