Answer:
53.18 grams of H₂SO₄ are needed to react with 78.86 grams of Al(NO₃)₃.
Explanation:
The balanced reaction between Al(NO₃)₃ and H₂SO₄ is:
2 Al(NO₃)₃ + 3 H₂SO₄ → Al₂(SO₄)₃ + 6 HNO₃
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reagents are required:
- Al(NO₃)₃: 2 moles
- H₂SO₄: 3 moles
Being the molar mass of the elements:
- Al: 27 g/mole
- N: 14 g/mole
- O: 16 g/mole
- H: 1 g/mole
- S: 32 g/mole
then the molar mass of the reactants are:
- Al(NO₃)₃: 27 g/mole + 3*(14 g/mole + 3*16 g/mole)= 213 g/mole
- H₂SO₄: 2*1 g/mole + 32 g/mole +4*16 g/mole= 98 g/mole
Then, by reaction stoichiometry, the following reagent mass amounts are required:
- Al(NO₃)₃: 2 moles* 213 g/mole= 436 g
- H₂SO₄: 3 moles*98 g/mole= 294 g
Then you can apply the following rule of three: If by stoichiometry 436 g of Al(NO₃)₃ react with 294 g of H₂SO₄, 78.86 g of Al(NO₃)₃ with how much mass of H₂SO₄ will it react?
mass of H₂SO₄=53.18 g
<u><em>53.18 grams of H₂SO₄ are needed to react with 78.86 grams of Al(NO₃)₃.</em></u>
Answer:
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Explanation:
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I would assume "cs" stands for centiseconds.
Using your metric prefixes...centi means one hundredth.
So 157 cs = 157 hundredths of a second = 1.57 seconds
Answer:
See explanation
Explanation:
We know that in the presence of strong oxidizing agents such as permanganate , aldehydes are oxidized. This oxidation is often accompanied by a colour change.
The colour change in the permanganate oxidation of benzaldehyde is caused by the inorganic permangate. The colour changes from purple to colourless because Mn^7+ is reduced to Mn^2+.
The benzaldehyde is readily oxidized to benzoic acid in the presence of permanganate.
The physical process of evaporation involves the heat absorbing and the status of the substance changing. The status of this substance changes form liquid to gas.