The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide.
I don't understand how to solve this, just want someone to explain. Thank you!
To determine the number of moles and the mass of oxygen formed by the decomposition of mercury(II) oxide, we need to use the concept of stoichiometry, which relates the quantities of reactants and products in a chemical reaction.
First, we need to know the balanced chemical equation for the decomposition of mercury(II) oxide. In this case, the reaction can be represented as:
2 HgO(s) -> 2 Hg(l) + O2(g)
According to the equation, 2 moles of mercury(II) oxide produce 1 mole of oxygen.
To find the number of moles of oxygen, we can use the given mass of mercury(II) oxide. The molar mass of mercury(II) oxide (HgO) can be found by summing the atomic masses of its constituent atoms: 200.59 g/mol for mercury (Hg) and 16.00 g/mol for oxygen (O).
Molar mass of HgO = 200.59 g/mol + 16.00 g/mol = 216.59 g/mol
Now we can calculate the number of moles of mercury(II) oxide:
Number of moles of HgO = Mass of HgO / Molar mass of HgO
Given mass of HgO = 1.252 g
Number of moles of HgO = 1.252 g / 216.59 g/mol = 0.00577 mol
Since the balanced chemical equation tells us that 2 moles of HgO produce 1 mole of O2, we can calculate the number of moles of oxygen formed:
Number of moles of O2 = Number of moles of HgO / 2
Number of moles of O2 = 0.00577 mol / 2 = 0.00289 mol
Finally, to find the mass of oxygen formed, we can use the molar mass of oxygen:
Mass of O2 = Number of moles of O2 x Molar mass of O2
Molar mass of O2 = 32.00 g/mol
Mass of O2 = 0.00289 mol x 32.00 g/mol = 0.0925 g
Therefore, the number of moles of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide is approximately 0.00289 mol, and the mass of oxygen formed is approximately 0.0925 g.
To find the number of moles and the mass of oxygen formed by the decomposition of mercury(II) oxide, we can use the balanced chemical equation for the decomposition reaction.
The balanced equation for the decomposition of mercury(II) oxide is:
2 HgO → 2 Hg + O2
From the equation, we can see that 2 moles of mercury(II) oxide decompose to form 1 mole of oxygen gas.
To find the number of moles of oxygen formed, we need to know the molar mass of mercury(II) oxide (HgO). The molar mass of HgO can be calculated by adding the atomic masses of its constituent atoms:
Molar mass of HgO = Atomic mass of Hg + Atomic mass of O
= (200.59 g/mol) + (16.00 g/mol)
= 216.59 g/mol
To find the number of moles, we can use the formula:
Number of moles = Mass of substance / Molar mass
Given that the mass of mercury(II) oxide is 1.252 g, we can calculate the number of moles:
Number of moles of HgO = 1.252 g / 216.59 g/mol
≈ 0.00578 mol
Since the coefficient of oxygen in the balanced equation is 1, we know that 1 mole of mercury(II) oxide decomposes to form 1 mole of oxygen.
Therefore, the number of moles of oxygen formed is also approximately 0.00578 mol.
To find the mass of oxygen formed, we can use the equation:
Mass = Number of moles x Molar mass
Mass of oxygen = 0.00578 mol x (32.00 g/mol) (molar mass of O2)
≈ 0.185 g
Therefore, the number of moles of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide is approximately 0.00578 mol, and the mass of oxygen formed is approximately 0.185 g.