Complete thedonechartworkx-X-( chemical thermodynamics)Iso thermal process :-Compression, w =o ReversibleExponsion,いニCompression, w=Irreversibl eい= ?Expansion,Adiabaticprocess :-Compression, w =O ReversibleExponsion,い=Compression, w=?Irreversibl eExpansion, w= ?® Isobaric processCompre ssion, w =?O ReversibleExponsion,い=Compression, w=IrreversibleExpansionWこ 2

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Complete the done chart work X- ( chemical thermodynamics) Iso thermal process :- Compression, w = o Reversible Exponsion, compression, ? Irreversibl e Expansion, w= ?

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 measure the energy of a solution phase reaction. Themeter Mod 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 92.55 grams of zinc to 97.73 °C and then drops it into a cup containing 78.30 grams of water at 21.37 °C. She measures the final temperature to be 28.88 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = 3/°C Submit Answer Retry Entire Group 8 more group attempts remaining
Please help me with the following question and explain it pls making sure its 100% correct. I keep getting this answer but it marks me wrong I am not sure whats wrong, pls help thank you
A bomb calorimeter is loaded with 1.465 g of caffeine (CgH1002N4; 184.19 g/mol) brated heat capacity of the ature was 23.50 °C. The and pressurized with excess oxygen. The previously calorimeter and contents is 3550 J/°C. The initial teu known internal energy of combustion of caffeine is -4251.4 kJ/mol. What is the final temperature after combustion? Report the temperature in °C with two decimal places but do not put units in the answer box.
Calculate the enthalpy of the following reaction: CH2 Hz(g) Cy44 (0 2C2H2() 502 4C02 ) D 2 H2O() M -1500 kj 2CzHalg) 602 4C02 (g)+ 4 H20(1) AH -1750 kj 2H2) Ozg) 2H20() AH -623 kj None of the above O 436.5 k/mol O 731.2 k/mol O 436.5 kl/mol O 870.5 k/mol
7(mheat)
The combustion of 0.150g of ethanol, CHOH(1) 2 5 releases 4.47kJ of heat. The molar enthalpy of combustion of liquid is?
3. Reversible adiabatic of a gas leads to (a) expansion, heating (b) compression, cooling (c) compression, no difference in the temperature (d) expansion, cooling of the system.
Which of the following statements is false? internal energy is a state function Ostate functions depend on the path taken O enthalpy is a state function O if a chemical or physical process is carried out at constant pressure with the only work done caused by expansion or contraction, then the heat flow (qp) and enthalpy change (AH) for the process are equal.
Heat Capacity We define q, the amount of (energy transferred as) heat as directly proportional to the temperature change (AT): q-CAT where C is a positive constant (called the heat capacity of the sample). We can see from this equation that the larger the temperature change is (for a given sample), the more heat must have been transferred. If AT-1° C, then q and C are numerically equal; thus, heat capacity can be defined as the amount of heat needed to cause a temperature change of 1 : °C By convention AT is calculated by subtracting the initial temperature from the final temperature. AT = Tfinal - Tinitiat %3D Therefore, for a sample that warmed up, the algebraic sign of ATis positive • and the algebraic sign of q is positive For a sample that cooled down, the algebraic sign AT is negative and the algebraic sign of q is negative If the temperature of a sample decreased from 20.00°C to 18.00°C, then (in degrees Celsius) is AT - 18,00 : "c- 20.00 : °C = 2.00 : C In Kelvin, AT -( 18.00 •…