Question

В баллоне 16л. 0.8 кг азота при т=310 К. при изохорном нагревании давление дост-ет 2.2*10^6 Па. определить начальное давление и конечную температуру

Answer 1

Только я понять не могу почему получилось начальное давление больше конечного...

Answer 2

Given Information

The initial volume of the container is 16 liters, and it contains 0.8 kg of nitrogen at a temperature of 310 K. During isochoric heating, the pressure reaches 2.2*10^6 Pa.

Solution

To solve for the initial pressure and the final temperature, we can use the ideal gas law equation:

PV = nRT

Where: - P = pressure - V = volume - n = number of moles - R = ideal gas constant - T = temperature

First, we need to calculate the initial number of moles of nitrogen using the given mass and molar mass of nitrogen.

Then, we can use the initial conditions to find the initial pressure. Finally, we can use the relationship between pressure and temperature during isochoric heating to find the final temperature.

Calculations

1. Calculate the number of moles of nitrogen: - The molar mass of nitrogen (N2) is approximately 28.02 g/mol. - Number of moles = mass / molar mass - Number of moles = 0.8 kg / 0.02802 kg/mol

2. Calculate the initial pressure: - Use the ideal gas law: PV = nRT - Rearrange the equation to solve for initial pressure: P = (nRT) / V

3. Calculate the final temperature: - Use the relationship between pressure and temperature during isochoric heating: P1 / T1 = P2 / T2

Results

1. Number of moles of nitrogen: - Number of moles = 0.8 kg / 0.02802 kg/mol - Number of moles ≈ 28.56 mol

2. Initial pressure: - Using the ideal gas law: P = (nRT) / V - Substituting the values, we can calculate the initial pressure.

3. Final temperature: - Using the relationship between pressure and temperature during isochoric heating: P1 / T1 = P2 / T2 - Substituting the known values, we can solve for the final temperature.

Let's calculate the values based on the given information.