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A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))
Correct answer is '14187'. Can you explain this answer?
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Verified Answer
A system filled with 0.505 mol of gas contracts reversibly from 1L to ...
q = -1270J
Even through process is isothermal but overall ΔU change is not zero. So. applying first law
ΔU = q + w = -1270 + 2688 = 14187
Even through process is isothermal but overall ΔU change is not zero. So. applying first law
ΔU = q + w = -1270 + 2688 = 14187
Most Upvoted Answer
A system filled with 0.505 mol of gas contracts reversibly from 1L to ...
In order to solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure of the gas (constant in this case)
V = Volume of the gas
n = Number of moles of gas
R = Ideal gas constant
T = Temperature of the gas (constant in this case)
We are given:
n = 0.505 mol (number of moles of gas)
V1 = 1L (initial volume of the gas)
V2 = 0.10L (final volume of the gas)
Since the temperature is constant, we can rewrite the ideal gas law equation as:
P1V1 = P2V2
Where:
P1 = Initial pressure of the gas
P2 = Final pressure of the gas
We need to find P2, the final pressure of the gas.
Rearranging the equation, we get:
P2 = (P1V1) / V2
Substituting the given values, we have:
P2 = (P1 * 1L) / 0.10L
Since the pressure is constant, P1 = P2.
P1 = P2 = (P1 * 1L) / 0.10L
Multiplying both sides by 0.10L, we get:
0.10L * P1 = P1 * 1L
Canceling out P1 on both sides, we have:
0.10L = 1L
Dividing both sides by 1L, we get:
0.10 = 1
This is not a valid conclusion, as it implies that 0.10 is equal to 1, which is not true.
Therefore, there must be an error in the problem statement or the calculations.
PV = nRT
Where:
P = Pressure of the gas (constant in this case)
V = Volume of the gas
n = Number of moles of gas
R = Ideal gas constant
T = Temperature of the gas (constant in this case)
We are given:
n = 0.505 mol (number of moles of gas)
V1 = 1L (initial volume of the gas)
V2 = 0.10L (final volume of the gas)
Since the temperature is constant, we can rewrite the ideal gas law equation as:
P1V1 = P2V2
Where:
P1 = Initial pressure of the gas
P2 = Final pressure of the gas
We need to find P2, the final pressure of the gas.
Rearranging the equation, we get:
P2 = (P1V1) / V2
Substituting the given values, we have:
P2 = (P1 * 1L) / 0.10L
Since the pressure is constant, P1 = P2.
P1 = P2 = (P1 * 1L) / 0.10L
Multiplying both sides by 0.10L, we get:
0.10L * P1 = P1 * 1L
Canceling out P1 on both sides, we have:
0.10L = 1L
Dividing both sides by 1L, we get:
0.10 = 1
This is not a valid conclusion, as it implies that 0.10 is equal to 1, which is not true.
Therefore, there must be an error in the problem statement or the calculations.
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A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer?
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A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer?.
A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))Correct answer is '14187'. Can you explain this answer?.
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