Question

A 0.0277m³container is initially evacuated. then, 7.54 g of water is placed in the container, and after some time, all of the water evapoartes. if the temperature of the water vapor is 352k, what is its pressure?

Answer 1

To find the pressure of water vapor in a container at 352 K, the ideal gas law is used. The mass of water is converted to moles and the values are plugged into the formula PV = nRT, resulting in a pressure of approximately 418185.6 N/m².

Step-by-step explanation:

To calculate the pressure of water vapor inside the container, we can use the ideal gas law which is PV = nRT. Here, P represents pressure, V is volume, n is the number of moles, R is the ideal gas constant (8.314 J/(mol·K)), and T is temperature in Kelvin.

First, we need to find the number of moles of water. This can be calculated by dividing the mass of water (7.54 g) by the molar mass of water (approximately 18.02 g/mol).

Number of moles (n) = 7.54 g / 18.02 g/mol = 0.418 mol.

Next, we plug all the values into the ideal gas law:

P = (nRT) / V.

So the pressure P = (0.418 mol * 8.314 J/(mol·K) * 352 K) / 0.0277 m³.

Calculating this we get:

P = 418185.6 N/m².

Therefore, the pressure of the water vapor in the container at 352 K is approximately 418185.6 N/m² or Pa.