There is an apparatus that consists of three glass bulbs connected by small glass tubes with the stopcocks closed. Given that the temp. is 27 degrees C, what is the pressure of gas in each glass bulb?

Bulb 1-> 1L- 1.79gCO2
Bulb 2-> 2L- 0.162gH2
Bulb 3-> 3L- 4.87gAr

A duplicate post.

To determine the pressure of gas in each glass bulb, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant, and T is the temperature in Kelvin.

First, we need to determine the number of moles for each gas in each bulb using the given masses and molar masses of the gases.

1. Calculate the number of moles of CO2 in Bulb 1:
- Molar mass of CO2 = 44.01 g/mol
- Moles of CO2 = mass of CO2 / molar mass of CO2
= 1.79 g / 44.01 g/mol

2. Calculate the number of moles of H2 in Bulb 2:
- Molar mass of H2 = 2.02 g/mol
- Moles of H2 = mass of H2 / molar mass of H2
= 0.162 g / 2.02 g/mol

3. Calculate the number of moles of Ar in Bulb 3:
- Molar mass of Ar = 39.95 g/mol
- Moles of Ar = mass of Ar / molar mass of Ar
= 4.87 g / 39.95 g/mol

Next, convert the temperature from degrees Celsius to Kelvin:
- Kelvin temperature = Celsius temperature + 273.15
= 27 + 273.15

Now that we have the number of moles and the temperature in Kelvin for each gas in the bulbs, we can use the ideal gas law to calculate the pressure.

1. For Bulb 1:
- Volume (V) = 1 L
- Moles (n) = obtained in step 1
- Temperature (T) = obtained by converting 27 degrees Celsius to Kelvin
- Solve for P: P = (n * R * T) / V

2. For Bulb 2:
- Volume (V) = 2 L
- Moles (n) = obtained in step 2
- Temperature (T) = obtained by converting 27 degrees Celsius to Kelvin
- Solve for P: P = (n * R * T) / V

3. For Bulb 3:
- Volume (V) = 3 L
- Moles (n) = obtained in step 3
- Temperature (T) = obtained by converting 27 degrees Celsius to Kelvin
- Solve for P: P = (n * R * T) / V

Remember to use the appropriate value for the gas constant, R, depending on the units you're using. The ideal gas constant in SI units is approximately 8.314 J/(mol·K).

By substituting the values into the equations, you should be able to calculate the pressure of gas in each glass bulb.