A system has an initial energy of 117 Joules. The energy equation includes -40.1 J of heat and 20.3 J of work. What is the final energy? Was heat added to the system or to the environment? Was work done the system or to the system? Be sure to show all of your work and include the correct units. by Use the paperclip button below to attach files.

A system has an initial energy of 117 Joules. The energy equation includes -40.1 J of heat and 20.3 J of work. What is the final energy? Was heat added to the system or to the environment? Was work done the system or to the system? Be sure to show all of your work and include the correct units. by Use the paperclip button below to attach files.

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

Use the following information to answer Questions 1-5: An aluminum sample weighing 31.1 g is placed in a hot water bath at 99.0 oC. The calorimeter contains 37.5 g of deoinized water. The initial temperature of the water is 18.5 oC. The metal is transferred to the calorimeter and the final temperature reached by the water, metal, and calorimeter is 28.6 oC. assume qmetal = -1710 J and qH2O = 1430 J. ΔTH2O = 10.1 oC. Calculate the calorimeter constant, Ccal in J/oC. Keep three sig figs in your answer.
An 18.89 g sample of neon gas in a container with a movable wall is initially at a temperature of 320 K and a pressure of 1.0 atm (which matches the external pressure of 1.0 atm). The container is then heated to 405 K, and its volume increases until its pressure is once again at 1.0 atm. How much work was done on the system in this process? Report your final answer in units of J.
18. An unknown volume of water at 18.2°C is added to 24.4 mL of water at 35.0°C. If the final temperature is 23.5°C, what was the unknown volume? (Assume no heat is lost to the surroundings; d of water = 1.00 g/mL)
A 2.5 g sample of french fries is placed in a calorimeter with 500.0 mL of water. The initial temperature of the water is 21.0 0C. After combustion of the french fries, the water has a temperature of 48.0 0C. Calculate the heat gained by the water (calories). Remember--the density of water is 1.00 g/mL. Report your answer to three significant figures
10. Ethanol OH weighing 3.56 g is burned in a calorimeter. The temperature rises from 15.C to C. The temperature rises from 15.1 If to 28. heat of the bomb plus water is 8.224C. Find the Δ in kJ/mol. (provide the given and required to find in the problem) (Kindly provide a CLEAR and COMPLETE solution) (Answer should be typewritten)
2. A 32.5g cube of aluminum initially at 45.8°C is submerged into 105.3 g of water at 15.4°C. The final temperature is 17.3°C. What is the heat capacity of aluminum? Swater = 4.184 J/g°C.
Please don't provide handwriting solution
A certain chemical reaction releases 13.4/kJg of heat for each gram of reactant consumed. How can you calculate the heat produced by the consumption of 3.2kg of reactant? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols.
A hot 122.8 g lump of an unknown substance initially at 154.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 56.9 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. graphite zinc aluminum titanium tungsten rhodium Substance Specific heat (J/(g-°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 0.132 0.388 4.184 tungsten zinc water
they are the part of one question. kindly do all A,B,C
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