Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2 (g)2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+ 3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 14.6 gg . Part A What minimum mass of H2SO4H2SO4 would you need? Express your answer in grams.

The minimum mass of H₂SO₄ that would be needed is 79.6 g

From the question,

We are to determine the minimum mass of H₂SO₄ required to dissolve 14.6 g of aluminum block.

The given balanced chemical equation for the reaction is

2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3H₂(g)

This means,

3 moles of sulfuric acid is required to dissolve 2 moles of Aluminum

First, we will determine the number of moles of aluminum present

From the given information,

Mass of aluminum block = 14.6 g

Using the formula

Atomic mass of aluminum = 26.98 g/mol

∴ Number of moles of Al present =

Number of moles of Al present = 0.54114 mole

Since

3 moles of sulfuric acid is required to dissolve 2 moles of Aluminum

Then,

x moles of sulfuric acid is required to dissolve 0.54114 mole of Aluminum

x =

x = 0.81171 mole

∴ The minimum number of mole of sulfuric acid required is 0.81171 mole

Now, for the minimum mass of sulfuric acid required

Using the formula

Mass = Number of moles × Molar mass

Molar mass of sulfuric acid = 98.079 g/mol

∴ Minimum Mass of sulfuric acid required = 0.81171 × 98.079

Minimum Mass of sulfuric acid required = 79.6117 g

Minimum Mass of sulfuric acid required ≅ 79.6 g

Hence, the minimum mass of H₂SO₄ that would be needed is 79.6 g

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76.3 g of H₂SO₄ are needed in this reaction

Explanation:

Let's begin with the reaction:

2Al(s) + 3H₂SO₄(aq)  →  Al₂(SO₄)₃ (aq)  +  3H₂(g)

Ratio in the reactants side is 2:3. It means that 2 moles of aluminum need 3 moles of sulfuric acid to react.

We determine the mass of Al → 14.6 g . 1mol / 26.98 g = 0.519 moles

Let's propose this rule of three:

2 moles of Al react with 3 moles of H₂SO₄

Then 0.519 moles of Al will react with (0.519 . 3) /2 = 0.778 moles of acid.

We convert the moles to mass, to find the

0.778 mol . 98 g / 1mol = 76.3 g

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.