Question

Баллон емкостью 0,5 л, содержащий воздух при нормальных условиях, герметически закрывают, после чего нагревают до температуры 400 С. Определить давление воздуха в баллоне при этой температуре. На сколько процентов увеличиться давление газа в нагретом сосуде, если перед герметизацией в него попадает 99 г воды?

Answer 1

5л умножить на 400+99

Answer 2

Calculation of Air Pressure in the Canister

To determine the air pressure in the canister after it is heated to a temperature of 400°C, we can use the ideal gas law. 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

Given that the canister has a volume of 0.5 L and contains air at normal conditions, we need to convert the temperature to Kelvin by adding 273.15 to the Celsius temperature. Therefore, the temperature in Kelvin is 400 + 273.15 = 673.15 K.

Since the canister is sealed, the number of moles of air remains constant. We can assume that the air behaves ideally, so we can rearrange the ideal gas law equation to solve for the pressure:

P = (nRT) / V

Substituting the known values into the equation:

P = (n * R * T) / V

Now, we need to find the number of moles of air in the canister. To do this, we can use the molar mass of air, which is approximately 28.97 g/mol. Since we know that the canister contains air at normal conditions, we can assume that the air is composed of approximately 78% nitrogen (N2) and 21% oxygen (O2) by volume.

To calculate the number of moles of air, we can use the following steps:

1. Calculate the mass of air in the canister: - The molar mass of air is 28.97 g/mol. - The volume of the canister is 0.5 L. - The density of air at normal conditions is approximately 1.225 kg/m³.

Using the formula: mass = density * volume, we can calculate the mass of air in the canister.

2. Calculate the number of moles of air: - Divide the mass of air by the molar mass of air.

Now, we can substitute the values of the number of moles of air, the ideal gas constant (R = 0.0821 L·atm/(mol·K)), the temperature in Kelvin, and the volume of the canister into the equation to calculate the pressure.

Let's perform the calculations:

1. Calculate the mass of air in the canister: - The density of air at normal conditions is approximately 1.225 kg/m³. - The volume of the canister is 0.5 L.

Using the formula: mass = density * volume, we can calculate the mass of air in the canister.

2. Calculate the number of moles of air: - Divide the mass of air by the molar mass of air.

3. Calculate the pressure using the ideal gas law equation: - Substitute the values of the number of moles of air, the ideal gas constant (R = 0.0821 L·atm/(mol·K)), the temperature in Kelvin, and the volume of the canister into the equation.

Let's perform the calculations:

1. Calculate the mass of air in the canister: - The density of air at normal conditions is approximately 1.225 kg/m³. - The volume of the canister is 0.5 L.

Using the formula: mass = density * volume, we can calculate the mass of air in the canister.

mass = 1.225 kg/m³ * 0.5 L * (1 m³ / 1000 L) = 0.0006125 kg

2. Calculate the number of moles of air: - Divide the mass of air by the molar mass of air.

moles of air = 0.0006125 kg / 0.02897 kg/mol = 0.02114 mol

3.