an alloy of metal A and B in the eatio of 2:5 and weighs 36g the percentage of metal A is 22.22% if atomic mass of A is 40 then atomic mass of metal B is
Well, well, well, looks like we have a little chemistry puzzle on our hands! Let's put on our thinking caps and solve it together, shall we?
Since the ratio of metal A to metal B in the alloy is 2:5, we can assume that there are 2 parts of metal A and 5 parts of metal B. This means that the total number of parts in the alloy is 2 + 5 = 7.
Now, if the percentage of metal A in the alloy is 22.22%, that means the weight of metal A is 22.22% of the total weight of the alloy. So, 22.22% of 36g is equal to (22.22/100) * 36 = 8g.
Since 2 parts of the alloy are made up of 8g of metal A, we can find the weight of 1 part of metal A by dividing 8g by 2, resulting in 4g.
Now, if we know that the atomic mass of metal A is 40, then the weight of 1 part of metal A (4g) is equal to the atomic mass of metal A (40).
So, to find the atomic mass of metal B, we can use the proportion:
Weight of 1 part of metal B / Atomic mass of metal B = Weight of 1 part of metal A / Atomic mass of metal A
Replacing the known values, we have:
Weight of 1 part of metal B / Atomic mass of metal B = 4g / 40
Dividing both sides of the equation by 4g, we get:
1 / Atomic mass of metal B = 1 / 10
And if we cross-multiply:
Atomic mass of metal B = 10
So, the atomic mass of metal B is 10.
Hope that explanation didn't leave you feeling metal-barrassed! Keep those chemistry questions coming!
To find the atomic mass of metal B, we need to calculate the total atomic mass of the alloy and determine the atomic mass of metal A.
1) Calculate the atomic mass of metal A:
If metal A is 22.22% of the alloy and weighs 36g, then the mass of metal A can be calculated as follows:
Mass of metal A = (22.22/100) * 36g = 7.998g
Since the atomic mass of metal A is given as 40, we can set up the following equation:
Atomic mass of metal A / Mass of metal A = 1 mole / 1 g
Rearranging the equation to find the atomic mass of metal A, we have:
Atomic mass of metal A = 1 mole / 1 g * Mass of metal A
Plugging in the values, we get:
Atomic mass of metal A = 1 mole / 1 g * 7.998g = 7.998 g/mol
2) Calculate the total atomic mass of the alloy:
Since the alloy is a mixture of metal A and metal B in a ratio of 2:5, and the percentage of metal A is 22.22%, we can calculate the percentage of metal B as follows:
Percentage of metal B = 100% - 22.22% = 77.78%
The percentage ratio of metal A to metal B is 2:5, so we can calculate the mass of metal B as follows:
Mass of metal B = (77.78/100) * 36g = 28.003g
Since we now know the mass of metal B, we can determine its atomic mass by setting up the following equation:
Atomic mass of metal B / Mass of metal B = 1 mole / 1 g
Rearranging the equation to find the atomic mass of metal B, we have:
Atomic mass of metal B = 1 mole / 1 g * Mass of metal B
Plugging in the values, we get:
Atomic mass of metal B = 1 mole / 1 g * 28.003g = 28.003 g/mol
Therefore, the atomic mass of metal B is 28.003 g/mol.
To find the atomic mass of metal B, we first need to calculate the mass of metal A and metal B in the given alloy.
Given:
Alloy ratio of metal A to metal B = 2:5
Total weight of the alloy = 36g
Percentage of metal A = 22.22%
Let's calculate the mass of metal A:
Mass of metal A = (Percentage of metal A / 100) * Total weight of the alloy
= (22.22 / 100) * 36g
= 7.99872g (rounded to 4 decimal places)
Now, let's calculate the mass of metal B:
Mass of metal B = Total weight of the alloy - Mass of metal A
= 36g - 7.99872g
= 28.00128g (rounded to 4 decimal places)
Next, we can find the number of moles of metal A and metal B by dividing their masses by their respective atomic masses:
Number of moles of metal A = Mass of metal A / Atomic mass of metal A
= 7.99872g / 40g/mol
= 0.199968 moles (rounded to 6 decimal places)
Number of moles of metal B = Mass of metal B / Atomic mass of metal B
Now, since we don't know the atomic mass of metal B yet, we'll denote it as 'x'.
Number of moles of metal B = 28.00128g / x (g/mol)
Since the alloy is made up of two parts metal A and five parts metal B, the ratio of their moles would be 2:5:
0.199968 moles (metal A) / 0.399936 moles (metal B) = 2/5
Simplifying this ratio:
0.199968 / 0.399936 = 2/5
Dividing both sides by 0.199968:
1 / 2 = (0.399936 / 0.199968) / 5
2 = 1.99984 / 5
2 = 2.99984 / x
Now, cross-multiply:
x = (2.99984 * 5) / 2
x = 7.4996
Therefore, the atomic mass of metal B is approximately 7.4996 g/mol.
If %A = 22.22%, then %B = 77.78.
Take 100 g sample to give you
22.22 g A
77.78 g B.
Convert to mols.
22.22/40 = 0.5555 mols A.
77.78/atomic mass B = ? mols B.
You know the ratio is A2B5; re-write this way letting X stand for atomic mass of B.
22.22/40 = 0.5555 x some # = 2
77.78/X = ? x some # = 5
We can calculate "some # from A.
2/0.5555 = 3.60 and we use that number to calculate ? from B. That will be 5/3.60 = 1.388. Now the B line reads
77.78/X = ? x 1.388 which allows us to calculate X as 77.78/1.388 = 56 for the atomic mass of B.
Check: If A2B5 is correct.
2*40 = 80
5*56 = 280
molar mass A2B5 = 360
%A = [80/360]*100 = 22.22
%B = [280/360]*100 = 77.78
Looks ok to me.