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

These all follow the general gas law which is PV = nRT.

To find n, use grams/molar mass. Don't forget to change T to Kelvin.

To find the pressure of gas in each glass bulb, we can use the Ideal Gas Law equation, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin. The temperature in Kelvin (T) can be calculated by adding 273.15 to Celsius temperature. In this case, T = 27 + 273.15 = 300.15 K.

Next, we need to determine the number of moles of gas in each bulb. We can use the formula:

n = m/M

where n is the number of moles, m is the mass of the gas, and M is the molar mass of the gas.

For Bulb 1, the mass of CO2 (m) is given as 1.79 g. The molar mass of CO2 is 44.01 g/mol (1 mole of CO2 = 12.01 g of carbon + 2 x 16 g of oxygen). We can calculate the number of moles:

n1 = m1/M1 = 1.79 g / 44.01 g/mol = 0.0407 mol

For Bulb 2, the mass of H2 (m) is given as 0.162 g. The molar mass of H2 is 2.02 g/mol (1 mole of H2 = 2 x 1.01 g). We can calculate the number of moles:

n2 = m2/M2 = 0.162 g / 2.02 g/mol = 0.0802 mol

For Bulb 3, the mass of Ar (m) is given as 4.87 g. The molar mass of Ar is 39.95 g/mol. We can calculate the number of moles:

n3 = m3/M3 = 4.87 g / 39.95 g/mol = 0.122 mol

Now we can find the pressure of gas in each glass bulb using PV = nRT.

For Bulb 1 (1L volume):
P1 * 1L = 0.0407 mol * 0.0821 atm L/mol K * 300.15 K
P1 = (0.0407 * 0.0821 * 300.15) / 1 L
P1 ≈ 0.997 atm

For Bulb 2 (2L volume):
P2 * 2L = 0.0802 mol * 0.0821 atm L/mol K * 300.15 K
P2 = (0.0802 * 0.0821 * 300.15) / 2 L
P2 ≈ 0.989 atm

For Bulb 3 (3L volume):
P3 * 3L = 0.122 mol * 0.0821 atm L/mol K * 300.15 K
P3 = (0.122 * 0.0821 * 300.15) / 3 L
P3 ≈ 1.006 atm

Therefore, the pressure of gas in each glass bulb is approximately:
Bulb 1: 0.997 atm
Bulb 2: 0.989 atm
Bulb 3: 1.006 atm