Answer:
2415.9g (corrected to 1 d.p.)
Explanation:
(Take the atomic mass of Ga=69.7 and S=32.1)
Assuming Ga is the limiting reagent (because the question did not mention the amount of sulphur burnt),
From the balanced equation, the mole ratio of Ga:Ga2S3 = 4: 2 = 2: 1, which means, every 2 moles of Ga burnt, 1 mole of Ga2S3 is produced.
Using this ratio, let y be the no. of moles of Ga2S3 produced,
y = 20.5 / 2
= 10.25 mol
Since mass = no. of moles x molar mass,
the mass of Ga2S3 produced = 10.25 x (69.7x2 + 32.1x3)
= 2415.9g (corrected to 1 d.p.)
Answer:
Oxygen needed for Stannous Oxide: 1.350g
Oxygen needed for Stannic Oxide: 2.710g
Explanation:
You're working with 10.00 grams of Tin mass for both Stannous Oxide and Stannic Oxide.
- 10.00 grams of Tin for Stannous Oxide is already 88.10% of the mass needed. You need to find how much 11.90% of Oxygen mass is needed to create the compound. Find a factor that you can multiply 88.10% by to get 100%
- 88.10 * x = 100
- Solve for x and you get 1.135
- Multiply that number by the mass of Tin (10.00 grams) to get the complete compound (Mixture of Tin and Oxygen).
- 10.00g * 1.135 = 11.35g (Tin + Oxygen)
- Subtract (Compound - Tin) to find Oxygen
- 11.35g - 10.00g = 1.350g (Oxygen)
Repeat the process with Stannic Oxide
- Find the factor that gets 78.70% to 100%
- 100/78.70 = 1.271
- Multiply by Tin mass
- 10.00g * 1.271 = 12.71g (Compound)
- Subtract Compound by Tin
- 12.71g - 10.00g = 2.710g (Oxygen)
Answer:
Hypoflorous acid, HOF
Explanation:
From the question, we're told that the helium atoms effuses 3 times than the said gas X.
We can determine the rate of effusion by using the formula
r is inversely proportional to 1/√M, where M is the molecular mass of the gas.
And also,
r is inversely proportional to 1/t, where t is the time taken for effusion.
From both formulas I listed, we can conclude that t is directly proportional to √M. And thus we proceed.
The molecular mass of Helium is 4.
tHe = tX/3, where tx is the time taken for the unknown gas X
As of yet, we don't know the molecular mass of X. Next, we say that
tX/tHe =√Mx/MHe
3 = √Mx/4
If we square both the sides, to remove the square root, we have
9 = Mx/4
Mx = 36
The molecular mass of the unknown gas X is 36.
