At a certain temperature and pressure, one liter of CO2 gas weighs 1.45 g. What is the mass of one liter of C4H10 gas at the same temperature and pressure?

To determine the mass of one liter of C4H10 gas at the same temperature and pressure, we need to use the ideal gas law equation and the molar mass of C4H10. The ideal gas law equation is:

PV = nRT

Where:
P = pressure (in Pascal or atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant
T = temperature (in Kelvin)

First, let's convert the given mass of CO2 to moles. We know that the molar mass of CO2 is approximately 44 g/mol. Using the equation:

moles = mass / molar mass

moles of CO2 = 1.45 g / 44 g/mol
moles of CO2 ≈ 0.033 mol

Since the volume is given as 1 liter, we can assume that the number of moles of C4H10 gas will be the same.

Now we need to find the molar mass of C4H10 (butane). C4H10 consists of 4 carbon (C) atoms and 10 hydrogen (H) atoms.

Molar mass of C4H10 = (4 × atomic mass of C) + (10 × atomic mass of H)

Using the atomic masses from the periodic table:
Molar mass of C4H10 = (4 × 12.01 g/mol) + (10 × 1.008 g/mol)
Molar mass of C4H10 ≈ 58.12 g/mol

Finally, we can calculate the mass of one liter of C4H10 gas:

mass of C4H10 = moles of C4H10 × molar mass of C4H10
mass of C4H10 ≈ 0.033 mol × 58.12 g/mol
mass of C4H10 ≈ 1.91 g

Therefore, the mass of one liter of C4H10 gas at the same temperature and pressure is approximately 1.91 grams.

To determine the mass of one liter of C4H10 gas at the same temperature and pressure, we need to use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, let's convert the given weight of CO2 gas (1.45 g) into moles. To do this, we need to know the molar mass of CO2, which is 44.01 g/mol. We can use this information to calculate the number of moles (n) of CO2 gas:

n = Mass of CO2 / Molar mass of CO2
n = 1.45 g / 44.01 g/mol
n ≈ 0.03298 mol

Now, since the volume remains constant (1 liter), the number of moles of C4H10 gas (n) will be the same as the number of moles of CO2 gas (n). We need to find the mass of C4H10, so we need to know its molar mass. The molar mass of C4H10 is:

Molar mass of C4H10 = (4 * Atomic mass of C) + (10 * Atomic mass of H)
Molar mass of C4H10 = (4 * 12.01 g/mol) + (10 * 1.01 g/mol)
Molar mass of C4H10 = 58.14 g/mol

With the number of moles (n) being the same for both CO2 gas and C4H10 gas, we can calculate the mass of C4H10 gas:

Mass of C4H10 = n * Molar mass of C4H10
Mass of C4H10 = 0.03298 mol * 58.14 g/mol
Mass of C4H10 ≈ 1.92 g

Therefore, the mass of one liter of C4H10 gas at the same temperature and pressure is approximately 1.92 grams.

1.9111

Equal volume of gases at the same T and P contain the same number of molecules (and mols).

mols CO2 = 1.45/44 = 0.03295
Then 0.03295 x molar mass C4H10 = ?