Hint: Absolute zero is the temperature at which the pressure of the gas equals to zero. The pressure of a perfect vacuum, a void or space which has no matter at all is known as absolute zero pressure. It is not possible factually as it is very hard to reach the situation of perfect vacuum and also maintain the same for time being.
Complete answer: Let us understand and answer the given question; Let us consider, one mole of gas in one litre of volume is present whose temperature is 0 K. Using ideal gas law, we can solve for pressure at that point. Given that, P = x atm V = 1 L n = 1 mole R = 0.0821 atmL/molK T = 0 K Thus, by ideal gas law, \[\begin{align} & PV=nRT \\ & P=\frac{nRT}{V}=\frac{1mol\times 0.0821atmL/molK\times 0K}{1L} \\ & P=0atm \\ \end{align}\]
Note: Do note that from the definition (actually, the name as well), we get a clear idea that the pressure will result as zero. But as it is asked to calculate or justify the same so without getting confused, we must solve what we know using the basics of gas laws.
As a seasoned expert in thermodynamics and gas laws, my extensive knowledge in the field allows me to delve into the intricacies of the concepts presented in the given article. I hold a comprehensive understanding of the theoretical foundations and practical applications of these principles, which is crucial for deciphering the complex relationships within the realm of gas behavior.
The article revolves around the concept of absolute zero, a point in temperature where the pressure of a gas reaches zero. Let's break down the provided information and elucidate each component with precision.
Absolute Zero Pressure:
The article rightly points out that absolute zero pressure is associated with the theoretical condition of a perfect vacuum—a void or space devoid of any matter. In practical terms, achieving this state is exceedingly challenging, making it more of a theoretical construct than a realizable phenomenon. The mention of perfect vacuum aligns with the idea that at absolute zero temperature, the pressure of the gas approaches zero.
Ideal Gas Law Application:
The article further employs the ideal gas law to calculate the pressure of a gas under specific conditions. The ideal gas law equation, (PV = nRT), relates pressure ((P)), volume ((V)), the number of moles ((n)), the ideal gas constant ((R)), and temperature ((T)).
Let's apply this law to the given scenario:
[P = \frac{nRT}{V}]
Given values:
(P) (pressure) = (x) atm (initially unspecified)
(V) (volume) = 1 L
(n) (moles) = 1 mole
(R) (ideal gas constant) = 0.0821 atmL/molK
(T) (temperature) = 0 K
Substituting these values into the equation yields:
While the concept of absolute zero pressure intuitively implies zero pressure, the article emphasizes the importance of utilizing the gas laws to rigorously calculate and justify the result. By applying the ideal gas law, the calculated pressure at absolute zero temperature indeed aligns with the expectation of zero pressure, reinforcing the theoretical notion of absolute zero in the context of gas behavior.
In summary, my expertise allows me to navigate through these complex concepts, ensuring a clear understanding of the theoretical constructs and their practical implications in the realm of gas laws and thermodynamics.
Hint: Absolute zero is the temperature at which the pressure of the gas equals to zero. The pressure of a perfect vacuum, a void or space which has no matter at all is known as absolute zero pressure.
If particles have no kinetic energy, then they are not moving and cannot cause any pressure inside their container. This is why absolute zero (0 K) is also where pressure equals zero.
Zero absolute temperature- Then, molecules will have zero energy and will stay stationary. They wont collide with container boundary and thus will exert no pressure.
The lowest pressures currently achievable in laboratory are about 1×10−13 torrs (13 pPa). However, pressures as low as 5×10−17 torrs (6.7 fPa) have been indirectly measured in a 4 K (−269.15 °C; −452.47 °F) cryogenic vacuum system. This corresponds to ≈100 particles/cm3.
In 1848, Lord Kelvin introduced the idea of absolute zero. This is the point at which the atoms in an object stop moving entirely and so can't get any colder. By extrapolating from experiments, Kelvin calculated that this point would be reached at -273°C.
A: The widely accepted boundary where space begins, which would also be the point where the air pressure is assumed to be zero, is called the Kármán line, which is located 100 km (62 mi) up.
Zero kelvin. 15 C , also known as absolute zero is the lowest temperature possible on the kelvin scale which is physically unattainable. Nothing can be colder than on the kelvin scale. According to the third law of thermodynamics, “ A system has entropy at if and only if the system is in the pure state.”
When body temperature drops, the heart, nervous system and other organs can't work as well as they usually do. Left untreated, hypothermia can cause the heart and respiratory system to fail and eventually can lead to death. Common causes of hypothermia include exposure to cold weather or immersion in cold water.
In other words, since atmospheric pressure at sea level is 14.7 PSIA, you subtract the PSIA of 14.7 from an atm pressure of 14.7 to equal zero PSIG (14.7 (PSIA) – 14.7 (atm) = 0).
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