Part BAn ideal gaseous reaction (which is a hypothetical gaseous reaction that conformsto the laws governing gas behavior) occurs at a constant pressure of 35.0 atm andreleases 66.3 kJ of heat. Before the reaction, the volume of the system was 7.00 LAfter the reaction, the volume of the system was 3.00 L. Calculate the totalinternal energy change, AE, in kilojoules.Express your answer with the appropriate units.► View Available Hint(s)AE=Submit0BμÅValueState functions versus path functionsUnits?S ▼Part CAn ideal gas (which is is a hypothetical gas that conforms to the laws governinggas behavior) confined to a container with a massless piston at the top. (Figure 2) Amassless wire is attached to the piston. When an external pressure of 2.00 atm isapplied to the wire, the gas compresses from 4.40 to 2.20 L. When the externalpressure is increased to 2.50 atm, the gas further compresses from 2.20 to 1.76 LIn a separate experiment with the same initial conditions, a pressure of 2.50 atmwas applied to the ideal gas, decreasing its volume from 4.40 to 1.76 L in one step.If the final temperature was the same for both processes, what is the differencebetween q for the two-step process and g for the one-step process in joules?Express your answer with the appropriate units.►View Available Hint(s)BHAValueSubmitP PearsonUnits?

“Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts for you. To get the remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.” SOlution for the Part -B From the question we have, Pressure = 35.0 atm Heat (q) = -66.3 KJ (negative sign indicates that the system releases the heat) Initial volume (V1) = 7.0 L Final Volume (V2) = 3.0 LFrom the first law of thermodynamics we have, ∆E = q+W where W is the work done and it is represented as, W = -P∆V=-PV2-V1=-35.0 atm (3.0 - 7.0)L=-35.0atm×(-4.0L)=140 atm L As we have 1 atm L = 101.3×10-3KJThen the work done will be,=WW = 140× 101.3×10-3KJ=14.18 KJSubstituting the values in the first law, ∆E = -66.3 KJ + 14.18 KJ=−52.12 KJ The required total internal energy ∆E change is found to be -52.12 KJ

Science

Chemistry

Part B An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 35.0 atm and releases 66.3 kJ of heat. Before the reaction, the volume of the system was 7.00 L . After the reaction, the volume of the system was 3.00 L. Calculate the total internal energy change, AE, kilojoules. Express your answer with the appropriate units. ►View Available Hint(s) ΔΕ = Submit μA Value Units ?

Part B An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 35.0 atm and releases 66.3 kJ of heat. Before the reaction, the volume of the system was 7.00 L . After the reaction, the volume of the system was 3.00 L. Calculate the total internal energy change, AE, kilojoules. Express your answer with the appropriate units. ►View Available Hint(s) ΔΕ = Submit μA Value Units ?

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

Measurements show that the energy of a mixture of gaseous reactants increases by 301. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that – 104. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic ? Is the reaction exothermic or endothermic? O endothermic
A 55.0 g sample of brass is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The brass sample starts off at 86.7 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 26.5 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to the correct number of significant digits. J 0- g-°C 0 x10 X thermometer. insulated container water sample a calorimeter
A 56.2 g sample of aluminum, which has a specific heat capacity of 0.897 J-g¹C¹, is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the aluminum sample. Be sure your answer is rounded to the correct number of significant digits. °C X Ś thermometer- insulated. container water sample a calorimeter
As a system increases in volume, it absorbs 55.0 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.540 atm. The final volume of the system is 58.2 L. What was the initial volume of the system if the internal energy of the system decreased by 103.4 J?
When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (CH-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 21.00 °C to 42.00 °C over a time of 8.5 minutes. Next, 5.190 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 21.00 °C to 63.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. exothermic C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g) Be…
A 56.5 g sample of iron is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The iron sample starts off at 86.7 °C and the temperature of the water starts off at 21.0 °C. When the temperature of the water stops changing it's 22.8 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2 significant digits. J 0₂-C x10 x thermometer insulated container water sample a calorimeter
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500. g of water (see sketch at right). First, a 6.500 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 18.00 °C to 44.66 °C over a time of 14.6 minutes. Next, 4.910 g of ethanol (C₂H5OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 40.44 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of…
Measurements show that the enthalpy of a mixture of gaseous reactants increases by 195.kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 69.kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. Is the reaction exothermic or endothermic?
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 7.500 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 18.00 °C to 51.74 °C over a time of 14.9 minutes. Next, 4.510 g of ethane (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 53.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ per mole of C₂H6.…
I A sample of aluminum, which has a specific heat capacity of 0.897 J.g .°C is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The aluminum sample starts off at 85.5 °C and the temperature of the water starts off at 16.0 °C. When the temperature of the water stops changing it's 23.3 °C. The pressure remains constant at 1 atm. Calculate the mass of the aluminum sample. Be sure your answer is rounded to the correct number of significant digits. thermometer. insulated container water sample a calorimeter