Question

V(O2) = 76лV(N2) = 84лV(CO₂) = 40лp(N2)-?​

Answer 1

Ответ:

получается 27

Объяснение:

так оно решается

Answer 2

To find the partial pressure of nitrogen gas (N2) in a mixture, you can use the ideal gas law, which states:

PV = nRT

Where:

• P is the pressure of the gas (in atmospheres, atm)
• V is the volume of the gas (in liters, L)
• n is the number of moles of the gas
• R is the ideal gas constant (approximately 0.0821 L·atm/(mol·K))
• T is the absolute temperature (in kelvin, K)

First, we need to find the number of moles of each gas using the given volumes and conditions:

For oxygen (O2): V(O2) = 76 L

For nitrogen (N2): V(N2) = 84 L

For carbon dioxide (CO2): V(CO2) = 40 L

Now, we can find the number of moles for each gas using the ideal gas law:

n(O2) = (V(O2) * P) / (R * T)

Since you haven't provided the temperature (T) or pressure (P), we can't calculate the number of moles directly for each gas. To find the partial pressure of nitrogen (p(N2)), you need to know the total pressure (P) and the mole fraction of nitrogen (X(N2)) in the mixture.

The mole fraction of nitrogen can be calculated as follows:

X(N2) = n(N2) / (n(O2) + n(N2) + n(CO2))

Once you have the mole fraction of nitrogen, you can find the partial pressure of nitrogen using the total pressure:

p(N2) = X(N2) * P

Please provide the values for the total pressure (P) and the temperature (T) so that we can calculate the partial pressure of nitrogen.