Answer is 273
explanation:
The rule of division for significant figures is to put the answer to the least amount of significant figures presented in the problem.
0.0131 only has 3 sig figs which is 131
3.582 has 4 sig figs
The least amount is 3 in the problem
When you originally divide 3.582 and 0.0131 you get 273.4531 in your calculator
Now put it to 3 sig figs
4 is not greater than 5 so you don't need to round
273 is 3 sig figs.
So answer is 273
Answer:
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The balanced equation for the reaction is as follows;
2H₂S + SO₂ —> 2H₂O + 3S
Stoichiometry of H₂S to SO₂ is 2:1
Limiting reactant is fully used up in the reaction and amount of product formed depends on amount of limiting reactant present.
Number of H₂S moles - 8.0 g / 34 g/mol = 0.24 mol of H₂S
Number of SO₂ moles = 12.0 g / 64 g/mol = 0.188 mol of SO₂
According to molar ratio of 2:1
If we assume H₂S to be the limiting reactant
2 mol of H₂S reacts with 1 mol of SO₂
Therefore 0.24 mol of H₂S requires - 1/2 x 0.24 = 0.12 mol of SO₂
But 0.188 mol of SO₂ is present therefore SO₂ is in excess and H₂S is the limiting reactant.
H₂S is the limiting reactant
Amount of S produced depends on amount of H₂S present
Stoichiometry of H₂S to S is 2:3
2 mol of H₂S forms 3 mol of S
Therefore 0.24 mol of H₂S forms - 3/2 x 0.24 mol = 0.36 mol of S
Mass of S produced = 0.36 mol x 32 g/mol = 11.5 g of S is produced
In every 100g of that compund there is 50.84 g of C, 8.53 g H and (100-59.37) g = 40.63 g of O.
Step 1: Convert each element's mass in moles. To do that we need to divide each element's mass by their respective molar mass.
For Carbon.
For Hydrogen.
For Oxygen.
Step 2: Divide each of the numbers by the smallest number.
For Carbon.
For Hydrogen.
For Oxygen.
Step 3: So the empirical formula will be.
But using decimal will be messy. So we multiply the numbers by 3. The right empirical formula will be.
Answer:
0.2 grams
Explanation:
The expression is already in decimal form! Hope this helps.
-Lei
