When 1.187g of a metallic oxide is reduced with excess hydrogen, 1.054g of the metal is produced. How do you determine what the metal oxide is?
Ok, so in order to identify the metal oxide, you first start by taking 1.187g-1.054 to find the g of O2. getting .133, you then determine the moles by dividing by mm of O2=.0083125. Then, because it is a metal oxide, multiply the moles of O2 by 2. Then take the 1.054g and divide it by .0083 to get 63.4, which is Copper.
Well, my metallic friend, here's a whimsical way to figure it out:
First, let's give the metallic oxide a name, like "Mystery Metal Oxide" (M.M.O for short, because abbreviations are cool). Now, we know that the M.M.O weighs 1.187g and when it gets cozy with hydrogen, it loses some weight and transforms into 1.054g of pure metal.
So, we aren't dealing with some magical alchemy here. It's all about those mathematical calculations. Let's do some number acrobatics!
To find the amount of oxygen in M.M.O, subtract the weight of the metal (1.054g) from the total weight of the oxide (1.187g): 1.187g - 1.054g = 0.133g.
Now, since oxygen is a pretty light element, it's not going to contribute much to M.M.O's hefty weight. So, we get to shine the spotlight on the metal! We divide the weight of the metal (1.054g) by its atomic weight to figure out how many moles of metal we have.
A little detective work leads us to Molesville. Say, for example, the atomic weight of the metal is 27 g/mol. Then, we can calculate the moles of metal: 1.054g / 27 g/mol ≈ 0.039 mol.
Now, we have the number of moles of metal. If you remember that a metal oxide always consists of 1 mole of metal for every mole of oxygen, we can conclude that there must also be 0.039 moles of oxygen in the M.M.O.
With this information, we can find the atomic weight of oxygen by dividing the weight of oxygen (0.133g) by the number of moles of oxygen (0.039 mol): 0.133g / 0.039 mol ≈ 3.41 g/mol.
Voila! Now we know that the atomic weight of oxygen in M.M.O is around 3.41 g/mol. Comparing this value to the atomic weight of oxygen in known oxide compounds, we can identify the metal oxide that fits the bill.
Remember, my metallic buddy, this was just a fun way to figure things out. In reality, it takes a bit more precision, but hey, who doesn't appreciate a little clowning around with numbers?
To determine what the metal oxide is, you can use the concept of stoichiometry.
Step 1: Determine the moles of metal produced.
To do this, divide the mass of the metal by its molar mass:
Moles of Metal = Mass of Metal / Molar Mass of Metal
Step 2: Determine the moles of oxygen in the metal oxide.
Since the metal is produced from the metal oxide, the oxygen content in the metal oxide has reacted with the hydrogen to form water. The excess hydrogen means that all of the oxygen has reacted, so the moles of oxygen in the metal oxide is the same as the moles of water produced.
Step 3: Determine the moles of water produced.
To do this, divide the mass of water by its molar mass:
Moles of Water = Mass of Water / Molar Mass of Water
Step 4: Determine the moles of oxygen in the metal oxide.
Since water has the chemical formula H2O and there are two moles of hydrogen in every mole of water, the moles of oxygen in the water is half the moles of water:
Moles of Oxygen = Moles of Water / 2
Step 5: Determine the molar mass of the metal oxide.
To do this, divide the mass of the metal oxide by the moles of oxygen:
Molar Mass of Metal Oxide = Mass of Metal Oxide / Moles of Oxygen
Now that you have the molar mass of the metal oxide, you can identify the metal oxide based on its molar mass and known properties of different metal oxides.
To determine the identity of the metal oxide, we need to use stoichiometry and the concept of molar ratios.
First, let's convert the masses given into moles by dividing them by the molar mass of the respective substances. The molar mass of the metallic oxide and the metal can be found on the periodic table or determined based on their formulas.
Molar mass of the metallic oxide = M1
Molar mass of the metal = M2
Moles of the metallic oxide = mass of metallic oxide (1.187g) / Molar mass of M1
Moles of the metal = mass of metal (1.054g) / Molar mass of M2
Next, we will determine the mole ratio of the metallic oxide and the metal based on the balanced chemical equation of the reduction reaction. This equation relates the number of moles of the reactants and products.
For example, let's assume the balanced chemical equation for the reduction of the metallic oxide is:
M1Oxide + H2 -> Metal + H2O
From the balanced equation, we can see that the mole ratio between the metallic oxide (M1Oxide) and the metal is 1:1. This means that for every mole of M1Oxide, we expect to produce one mole of the metal.
Now, we can set up an equation using the mole ratios to find the molar mass of the metal oxide (M1):
Moles of M1Oxide / Moles of metal = Molar mass of M1Oxide / Molar mass of metal
Given the moles of the metallic oxide (calculated earlier) and the moles of the metal (value provided in the question), we can rearrange the equation to solve for the molar mass of M1Oxide:
Molar mass of M1Oxide = (Moles of M1Oxide / Moles of metal) * Molar mass of metal
By substituting the known values (masses and/or molar masses) into the equation, you can calculate the molar mass of the metallic oxide (M1Oxide). Finally, with the molar mass, you can search for the corresponding metal oxide formula using periodic tables or other references.