Question

Газ, объём которого 0.8 м в кубе при температуре 300к производит давление 2.8*10 в 5ой степени Па. определить приращение темепературы той же массы газа, если при давлении 1.6*10 в 5ой степени Па он занял обём 1.4м в кубе.......решите пожалуйста

Answer 1

по уравнению Менделеева-Клапейрона:

p₁*v₁/t₁=p₂*v₂/t₂

все. дальше выразить T₂.

Answer 2

Problem Statement

We are given a gas with a volume of 0.8 m³ at a temperature of 300 K, which produces a pressure of 2.8 * 10^5 Pa. We need to determine the change in temperature of the same mass of gas when it occupies a volume of 1.4 m³ at a pressure of 1.6 * 10^5 Pa.

Solution

To solve this problem, we can use the ideal gas law, which states that the pressure of a gas is directly proportional to its temperature and inversely proportional to its volume, assuming constant mass. The ideal gas law equation is given by:

PV = nRT

Where: - P is the pressure of the gas - V is the volume of the gas - n is the number of moles of gas - R is the ideal gas constant - T is the temperature of the gas in Kelvin

Since we are dealing with the same mass of gas, the number of moles (n) remains constant. Therefore, we can rewrite the equation as:

P₁V₁/T₁ = P₂V₂/T₂

Where: - P₁ and V₁ are the initial pressure and volume of the gas - T₁ is the initial temperature of the gas - P₂ and V₂ are the final pressure and volume of the gas - T₂ is the final temperature of the gas

We can rearrange the equation to solve for T₂:

T₂ = (P₂V₂ * T₁) / (P₁V₁)

Now, let's substitute the given values into the equation and calculate the final temperature.

Given: - P₁ = 2.8 * 10^5 Pa - V₁ = 0.8 m³ - T₁ = 300 K - P₂ = 1.6 * 10^5 Pa - V₂ = 1.4 m³

Substituting these values into the equation, we get:

T₂ = (1.6 * 10^5 Pa * 1.4 m³ * 300 K) / (2.8 * 10^5 Pa * 0.8 m³)

Calculating this expression, we find:

T₂ ≈ 300 K

Therefore, the change in temperature of the gas is approximately 0 K.

Please note that the given sources did not provide direct information for this specific problem. However, the solution is derived from the ideal gas law, which is a fundamental concept in thermodynamics and can be found in various physics and chemistry textbooks.