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3 years ago

How many moles of H 2 can be formed if a 3.24 g sample of M g reacts with excess H C l ?

Chemistry

1 answer:

Ganezh [65]3 years ago

3 0

Answer:

0.135 mole of H2.

Explanation:

We'll begin by calculating the number of mole in 3.24 g of Mg. This can be obtained as follow:

Mass of Mg = 3.24 g

Molar mass of Mg = 24 g/mol

Mole of Mg =?

Mole = mass /Molar mass

Mole of Mg = 3.24/24

Mole of Mg = 0.135 mole

Next, we shall write the balanced equation for the reaction. This is illustrated below:

Mg + 2HCl —> MgCl2 + H2

From the balanced equation above,

1 mole of Mg reacted to produce 1 mole of H2.

Finally, we shall determine the number of mole of H2 produced by reacting 3.24 g (i.e 0.135 mole) of Mg. This can be obtained as follow:

From the balanced equation above,

1 mole of Mg reacted to produce 1 mole of H2.

Therefore, 0.135 mole of Mg will also react to produce 0.135 mole of H2.

Thus, 0.135 mole of H2 can be obtained from the reaction.

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According to table g, which substance forms an unsaturated solution when 80. grams of the substance are stirred into 100. grams

e-lub [12.9K]

A saturated solution is one in which no more solute is able to dissolve in a given solvent at a particular temperature. Some amount of the solute is left undissolved in the solution.

Unsaturated solution has solute in lower proportions than required to form a saturated solution.

Supersaturated solution has solute in amounts greater than a saturated solution.

We can take the help of solubility curve in order to find out the amount of a salt required to prepare a saturated solution of that salt at a particular temperature.

The solubility of KI at 10 $^{0}C$ is 136 g/ 100 mL water

The solubility of $KNO_{3}$ at $10^{0}C$ is 21 g/100 mL water.

The solubility of $NaNO_{3}$ at $10^{0}C$ is 80 g/100 mL water.

The solubility of NaCl at $10^{0}C$ is 38 g/ 100 mL water.

So the correct answer will be KI, as it would need 136 g KI / 100 mL water to form a saturated solution at $10^{0}C$ .So, if we have 80g KI/ 100mL water it would be an unsaturated solution.

4 0

3 years ago

Read 2 more answers

Combustion reactions are exothermic. The heat of reaction for the combustion of 2-methylheptane, C8H18, is 1.306×103 kcal/mol. W

WARRIOR [948]

Answer:

11.45kcal/g

2.612 × 10³ kcal

Explanation:

When a compound burns (combustion) it produces carbon dioxide and water. The combustion of 2-methylheptane can be represented by the following balanced equation:

2 C₈H₁₈ + 25 O₂ ⇄ 16 CO₂ + 18 H₂O

It releases 1.306 × 10³ kcal every 1 mol of C₈H₁₈ that is burned.

What is the heat of combustion for 2-methylheptane in kcal/gram?

We know that the molar mass of C₈H₁₈ is 114.0g/mol. Then, using proportions:

$\frac{1.306 \times 10^{3}Kcal}{1mol} .\frac{1mol}{114.0g} =11.45kcal/g$