Question

In: Chemistry

8.2 Kj of heat is added to a system that expands from 3.00L to 6.00L against...

8.2 Kj of heat is added to a system that expands from 3.00L to 6.00L against 3.5 atm of pressure. Compute the delta E

Solutions

Expert Solution

Ans : AS per the first law of thermodynamics the energy can neither be created nor destroyed but it can only be transformed from one form to another .energy of an isolated system is always constant.

mathematical expression for first law of thermodynamics can be written as:

where Is the change in internal energy ,q is the heat and w is the work done by the system.

when work is done by the system it is denoted by the negative sign.w= -P

so,in the question we are having the heat added and the volume change in the system from 3 L to 6 L,pressure given is 3.5 atm.now put the values in the formula given above in solution and we get:

put w as -P (V=V2-V1)

= 8.2 - 3.5(6-3)

= 8.2-3.5*3

=8.2-10.5

=-2.3kJ

The negative change means that the final energy is less than the initial energy.

We were unable to transcribe this image

We were unable to transcribe this image

We were unable to transcribe this image

We were unable to transcribe this image

We were unable to transcribe this image

We were unable to transcribe this image

We were unable to transcribe this image

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

a) Find q, w , ∆E when a system gains 10.0 kJ of heat from the...
a) Find q, w , ∆E when a system gains 10.0 kJ of heat from the surroundings and does 14.0 KJ of work on the surroundings. b) If the standard enthalpy of reaction , ∆Ho , is -137.0 kJ for the chemical reaction C2H4(g) + H2(g) → C2H6(g) How much heat is liberated when 400.0 g of C2H6 is produced ? c) Given the following thermochemical reactions: CH4 (g) + 1/2 O2(g) → CH3OH (l) ∆Ho = -163.9 kJ CO2...
A system releases 65 kJ of heat and receives 82 kJ of work. What is ∆E?...
A system releases 65 kJ of heat and receives 82 kJ of work. What is ∆E? Is the process endothermic or exothermic?
8630 kJ of heat is added to 2.84 kg ice initially at -5.00°C. What is the...
8630 kJ of heat is added to 2.84 kg ice initially at -5.00°C. What is the final temperature of the resulting water (whatever state it may be in)?
A heat engine operates by extracting 2,000 KJ of heat from a source at 1500 K,...
A heat engine operates by extracting 2,000 KJ of heat from a source at 1500 K, and dumping 800 of waste heat into a sink at 300 K. a) Does this engine violate any known laws of thermodynamics? b) How much work does this engine produce? c) What are the first and second law efficiencies?
A heat engine receives an amount of energy Qh= 790 kJ by heat transfer from a...
A heat engine receives an amount of energy Qh= 790 kJ by heat transfer from a high temperature thermal reservoir at Th=950 K. Energy is rejected by heat transfer to a lower temperature thermal reservoir at T1=590 K. If waste heat in the amount of Q1=160 kJ is rejected to the low temperature thermal reservoir during each cycle. a) Solve for the maximum theoretical efficiency that an engine in this situation could operate with. ANSWER: 0.379 b) Solve for actual...
If a substance has a heat of condensation of –1.46 kJ/g and a heat of sublimation...
If a substance has a heat of condensation of –1.46 kJ/g and a heat of sublimation of 4.60 kJ/g, what is its heat of solidification in kJ/g? Answer: 1.46-4.60 kJ/g can you explain me why the asnwer is 1.46-4.60 kJ/g
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of...
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -10 ∘C. Please show work
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of...
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -14 ∘C. I feel like I should be able to get this problem but something is just not clicking. Thank you for your help!
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of...
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -13 ∘C.
Heat of Combustion and Enthalpy The heat of combustion of hexane is 45.6 kj/g. If you...
Heat of Combustion and Enthalpy The heat of combustion of hexane is 45.6 kj/g. If you burn all of a 1.20 g sample of hexane, and all of the heat is transferred to a pot of water determine the following: (a)The amount of heat in J, and the sign of the energy change (b)The amount of heat absorbed in water: (c) The final temperature of water if there are 250 g of water in the pot, and the intial water...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT