Elemental mercury was first discovered when a mercury oxide was decomposed with heat, forming mercury metal and oxygen gas. When a 0.204-g sample of the mercury oxide is heated, 0.189 g of mercury metal remains.
a)what is mole ratio of mercury to oxygen in the sample?
would it be
0.204 g x mol Hg/200.59= 0.001
0.189 g x mol Hg/200.59= 9.422204497E^-4
am confused don't know how to solve further.
&
b) what will be the empirical formula for mercury oxide?
please help thnk :)
HgO ==> Hg + O2
0.204...0.189..0.015
Remember the law of conservation of mass. The stuff on the right must add up to the stuff on the left.
Your mol Hg is correct at 0.000942
mol O2 = 0.015/32 = 0.000469
Then 0.000942/0.000469 = 2.008 which rounds to 2Hg to 1 oxygen.
So the ratio of mercury to oxygen will be 2:1 and how can find the empirical formula please...thank you
The ratio of Hg to O2 is 2:1.
The ratio of Hg to O(atom) is 1:1
Formula is HgO.
0.189/0.000942
0.150/16 = 0.00094375
ratio is 1:1 formula HgO.
A: To find the mole ratio of mercury to oxygen, you need to calculate the moles of mercury and oxygen separately.
First, calculate the moles of mercury remaining:
Moles of mercury = mass of mercury / molar mass of mercury
Moles of mercury = 0.189 g / 200.59 g/mol
Next, calculate the moles of oxygen consumed:
Moles of oxygen = (initial moles of mercury oxide) - (moles of mercury remaining)
The initial moles of mercury oxide can be calculated by assuming that the mass of the mercury oxide used is equal to the mass of mercury and oxygen combined:
Moles of mercury oxide = mass of mercury oxide / molar mass of mercury oxide
Moles of mercury oxide = 0.204 g / molar mass of mercury oxide
Since the molar mass of mercury(II) oxide (HgO) is 216.59 g/mol, you can substitute this value into the equation above to find the initial moles of mercury oxide.
Now you can calculate the mole ratio:
Mole ratio of mercury to oxygen = moles of mercury / moles of oxygen
B: To determine the empirical formula for mercury oxide, you need to know the ratio of mercury to oxygen atoms in the compound. From the mole ratio obtained in part A, you can determine this ratio. The empirical formula represents the simplest, most reduced ratio of elements in the compound.
Let's say the mole ratio of mercury to oxygen is x:y. This means that in the empirical formula of mercury oxide, there are x atoms of mercury for every y atoms of oxygen. To find the empirical formula, you need to simplify this ratio to its simplest whole number values.
For example, if the mole ratio is 1:1, then the empirical formula would be HgO. If the mole ratio is 2:1, then the empirical formula would be Hg2O.
To determine the empirical formula, divide both x and y by their greatest common divisor to obtain the simplest whole number ratio.
To solve part a) of the question, you are on the right track by using the mole ratio. Here's how you can proceed:
1) Calculate the number of moles of mercury remaining:
Moles of mercury = mass of mercury remaining (g) / molar mass of mercury (g/mol)
Moles of mercury = 0.189 g / 200.59 g/mol = 0.0009422204497 mol
2) Calculate the number of moles of oxygen that was initially present:
Moles of oxygen = Moles of mercury x (Moles of oxygen / Moles of mercury)
The ratio of moles of oxygen to moles of mercury can be determined from the balanced chemical equation. Since the equation is not provided, let's assume it is:
2 HgO -> 2 Hg + O2
From this equation, we can see that the mole ratio of mercury to oxygen is 2:1. Therefore, there are 0.0009422204497 mol of oxygen.
So, the mole ratio of mercury to oxygen in the sample is 1:0.0009422204497 or approximately 1:0.001.
Moving on to part b) of the question, to determine the empirical formula, we need to find the ratio of atoms present in the compound.
1) Determine the moles of mercury in the sample:
Moles of mercury = mass of mercury remaining (g) / molar mass of mercury (g/mol)
Moles of mercury = 0.189 g / 200.59 g/mol = 0.0009422204497 mol
2) Determine the moles of oxygen in the sample:
Moles of oxygen = Moles of mercury x (Moles of oxygen / Moles of mercury)
Using the same ratio of 2:1 from the balanced chemical equation, we can determine the moles of oxygen to be 0.0009422204497 mol.
3) Divide the number of moles of each element by the smaller number of moles:
0.0009422204497 mol mercury / 0.0009422204497 mol = 1
0.0009422204497 mol oxygen / 0.0009422204497 mol = 1
Based on these calculations, the empirical formula for mercury oxide is HgO.