How many molecules of CO2 are in 132.03 grams of CO2 ?

3.00 molecules

Explanation:

Given that:

Mass of CO2 = 132.03 grams

Number of molecules of CO2 = ?

Molar mass of CO2 = ?

For the molar mass of CO2: Atomic mass of Carbon = 12; Oxygen = 16

= 12 + (16 x 2)

= 12 + 32 = 44g/mol

Apply the formula:

number of molecules = (mass in grams/molar mass)

N = (132.03 grams/44g/mol)

N = 3.00 molecules

Thus, there are 3.00 molecules of CO2 in 132.03 grams of CO2.

*tilts head* sounds more like a statement

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm