You have two flasks of equal volume. Flask A contains H2 at 0°C and 1 atm pressure. Flask B contains CO2 gas at 0°C and 2 atm pressure. Compare these two gases with respect to each of the following

mass of gas (Flask A:Flask B)

The long way, which may be the best for beginners, is to use PV = nRT. Substitute and solve for n = number of mols; then mols = grams/molar mass. You know mols and molar mass, solve for grams and you have your answer.

its suppose to be a ratio

To compare the mass of gas in Flask A and Flask B, we can use the ideal gas law, which states:

PV = nRT

where:
P = pressure of the gas
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant
T = temperature in Kelvin

Given that the volumes of the flasks are equal and the temperatures are the same (0°C = 273.15 K), we can compare the masses of the gases using the equation:

n = (PV) / (RT)

Let's calculate the mass of gas in Flask A and Flask B separately.

For Flask A:
Pressure (P) = 1 atm
Volume (V) = same as Flask B
Temperature (T) = 0°C = 273.15 K

For Flask B:
Pressure (P) = 2 atm
Volume (V) = same as Flask A
Temperature (T) = 0°C = 273.15 K

To compare the masses, we need to calculate the number of moles (n) for both gases using the ideal gas law equation. Then, we can compare the moles to find the ratio of their masses.

Let's assume the volume of both flasks is V liters.

For Flask A:
n_A = (P_A * V) / (R * T)
= (1 atm * V) / (0.0821 L*atm/mol*K * 273.15 K)
= (V) / (22.414 L/mol) (rounded to two decimal places)

For Flask B:
n_B = (P_B * V) / (R * T)
= (2 atm * V) / (0.0821 L*atm/mol*K * 273.15 K)
= (2V) / (22.414 L/mol) (rounded to two decimal places)

Now, let's compare the masses of the gases in Flask A and Flask B:

Mass of gas in Flask A : Mass of gas in Flask B
= n_A : n_B
= (V) / (22.414 L/mol) : (2V) / (22.414 L/mol)
= V : 2V
= 1 : 2

Therefore, the mass of gas in Flask A is half the mass of gas in Flask B.

To compare the mass of gas in Flask A and Flask B, we need to use the Ideal Gas Law equation, which states:

PV = nRT

Where:
P = Pressure of the gas
V = Volume of the gas
n = Number of moles of the gas
R = Ideal gas constant
T = Temperature of the gas in Kelvin

Since the flasks have equal volumes, we can ignore the volume term in the equation. Let's assume we have 1 mole of each gas.

For Flask A:
Pressure (P) = 1 atm
Temperature (T) = 0°C = 273.15 K

For Flask B:
Pressure (P) = 2 atm
Temperature (T) = 0°C = 273.15 K

Now, we can calculate the number of moles (n) of each gas using the given conditions. Since we are assuming 1 mole of each gas, the number of moles will be the same for both gases.

n = 1 mole

Next, we can rearrange the Ideal Gas Law equation to solve for the mass (m) of the gas:

PV = nRT

m = (n × M) / V

Where:
m = mass of the gas
M = molar mass of the gas
V = volume of the gas

The molar mass of hydrogen gas (H2) is 2 g/mol and carbon dioxide gas (CO2) is 44 g/mol.

For Flask A (H2):
m = (1 mole × 2 g/mol) / V

For Flask B (CO2):
m = (1 mole × 44 g/mol) / V

Since the volumes of the flasks are equal, we can simplify the comparison by canceling out the volume term:

m (Flask A) : m (Flask B) = (2 g/mol) : (44 g/mol)
m (Flask A) : m (Flask B) = 1 : 22

Therefore, the mass of gas in Flask A is 1/22 times the mass of gas in Flask B.