Answer:
0.16mole
Explanation:
To solve this problem, we are going to assume that the number of moles of carbon to be determined is that at STP, standard temperature and pressure.
The number of moles of a substance at STP is given as;
Number of moles =
Given volume = 3.5L
Now, insert the parameters;
Number of moles = = 0.16mole
Dalton's atomic theory was based on the law of conservation of mass which states that the matter can neither be created nor be destroyed but it can only transformed into one form or another. In a chemical reaction, total mass of the reactants will be equal to the total mass of the products.
Taking an example,
Mass of = 16g
Mass of =
Total mass on reactant side =
Total mass on reactant side = 80g
Mass of = 44g
Mass of
Total mass on product side =
Total mass on product side = 80g
It is seen from the above example that the
total mass on reactant side = total mass on product side.
The question is incomplete, complete question is ;
A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.8 g of and 33.1 g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 21°C.Express the pressures in atmospheres to three significant digits separated by commas.
Answer:
Partial pressure of the oxygen gas is 3.91 atm.
Partial pressure of the helium gas is 20.0 atm
Total pressure of the gases is 24.0 atm
Explanation:
Moles of oxygen gas =
Moles of helium gas =
Total moles of gas =
Volume of the cylinder = V = 10.0 L
Total pressure in the cylinder = P = ?
Temperature of the gas in cylinder = T = 21°C = 21 + 273 K = 294 K
PV = nRT ( ideal gas equation )
P = 23.88 atm ≈ 23.9
Partial pressure of the individual gas will be determined by the help of Dalton's law:
partial pressure = Total pressure × mole fraction of gas
Partial pressure of the oxygen gas
Partial pressure of the helium gas