As variáveis temperatura, pressão e densidade, conhecidas como variáveis de estado, são relacionadas, nos gases, pela chamada lei dos gases ideais. Por definição, um gás ideal segue exatamente a teoria cinética dos gases, isto é, um gás ideal é formado de um número muito grande de pequenas partículas, as moléculas, que têm um movimento rápido e aleatório, sofrendo colisões perfeitamente elásticas, de modo a não perder quantidade de movimento.

A resposta correta é a letra D).

Para encontrar a pressão final do gás, the ideal, gas law should be used, equation, which relates the variables of state: temperature, pressure, and density. The ideal gas law is given by:

$$ PV = nRT $$, where n is the number of moles of gas, R is the gas constant, T is the temperature in Kelvin, P is the pressure, and V is the volume.

Given the initial conditions: P = 10 atm, V = 10 L, and T = 20°C = 293 K. We need to find the final pressure P when the temperature is increased to 50°C = 323 K, and the volume is reduced to 8 L.

First, we need to find the number of moles of gas n. Using the ideal gas law, we can rearrange the equation to solve for n:

$$ n = frac{PV}{RT} $$

Substituting the initial conditions, we get:

$$ n = frac{(10)(10)}{(8.314)(293)} = 0.041 mol $$

Now, we can use the ideal gas law again to find the final pressure P when the temperature is 323 K and the volume is 8 L:

$$ P = frac{nRT}{V} = frac{(0.041)(8.314)(323)}{8} = 13.45 atm $$

Therefore, the correct answer is D) 13.45 atm.

Explanation:

The ideal gas law is a fundamental equation in thermodynamics that relates the variables of state of an ideal gas. By using this equation, we can solve for the final pressure of the gas when the temperature and volume are changed. In this problem, we first found the number of moles of gas using the initial conditions, and then used the ideal gas law again to find the final pressure.