Question

Fe+O2–>Fl2O3 а)m(Fe)=28г б)V(O2)=?

Answer 1

Такие задачи решаются с помощью уравнения

Answer 2

To determine the volume of oxygen gas consumed in the reaction, we first need to balance the chemical equation:

4Fe + 3O2 -> 2Fe2O3

From the balanced equation, we can see that 3 moles of oxygen are required to react with 4 moles of iron. We can use this stoichiometry to calculate the volume of oxygen gas consumed based on the mass of iron used.

a) m(Fe) = 28 g The molar mass of iron (Fe) is 55.85 g/mol, so 28 g of iron corresponds to:

n(Fe) = m(Fe) / M(Fe) = 28 g / 55.85 g/mol = 0.501 mol

According to the balanced equation, 4 moles of iron react with 3 moles of oxygen, so the amount of oxygen required is:

n(O2) = 3/4 * n(Fe) = 3/4 * 0.501 mol = 0.376 mol

b) To calculate the volume of oxygen gas consumed, we need to know the conditions of the reaction (temperature, pressure, etc.) and use the ideal gas law. Assuming standard temperature and pressure (STP), which are 0°C (273.15 K) and 1 atm, respectively, we can use the molar volume of a gas at STP, which is 22.4 L/mol:

V(O2) = n(O2) * Vm(STP) = 0.376 mol * 22.4 L/mol = 8.4224 L

Therefore, the volume of oxygen gas consumed in the reaction is approximately 8.42 L at STP.