Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg + N2 → Mg3N2 In a particular experiment, a 9.27-g sample of N2 reacts completely. The mass of Mg consumed is __________ g.

Answer:

33.21% is the right answer.

Explanation:

0.04720 L * 0.02240 mol / L = 1.0573*10-3

mol Fe+2 = 1.0573* 10-3 mol = 5.2864*10-3

mass of Fe= 5.2864 * 10-3  = 0.29522g

% of Fe in sample = 0.29522 g Fe / 0.8890 g of sample * 100 = 33.21%

Final answer:

The number of moles of MnO4– added to the solution is 0.00106 mol. The moles of Fe2+ in the sample is 0.00530 mol. The grams of iron in the sample is 0.296 g and the percentage of iron in the sample is 33.33%.

Explanation:

The titration reaction between Fe2+ and MnO4– in acid solution is as follows: 5Fe2+ + MnO4– + 8H+ → 5Fe3+ + Mn2+ + 4H2O. Firstly, we can calculate the number of moles of MnO4– added to the solution using the formula volume X molarity. That is 0.0472 L X 0.02240 M = 0.00106 mol MnO4–. According to the balanced redox reaction, one mole of MnO4– reacts with five moles of Fe2+. Therefore, the moles of Fe2+ in the sample is 0.00106 mol MnO4– X 5 = 0.00530 mol Fe2+.

Next, we calculate the grams of iron in the sample. The molarmass of iron is approximately 55.85 g/mol, thus the grams of iron in the sample are 0.00530 mol Fe2+ X 55.85 g/mol = 0.296 g Fe2+. Finally, we find the percentage of iron in the sample by mass = (mass of iron in the sample / total mass of the sample) X 100%. Therefore, the percentage is (0.296 g / 0.8890 g) X 100% = 33.33%.

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Answer:

• The third chice: 0.0750 M Na₂SO₄

Explanation:

Assume 100% ionization:

1) 0.100 M solution K₂SO₄

• K₂SO4 (aq) → 2K⁺ (aq) + SO₄²⁻ (aq)

• Mole ratios: 1 mol K₂SO4 : 2 mol K⁺  + 1 mol SO₄²⁻ (aq) : 3 mol ions. This is 1 : 3

• At constant volume, the mole ratios are equal to the concentration ratios (M).

• 1  M K₂SO₄: 3 M ions = 0.100 M K₂SO₄ / x ⇒ x = 0.300 M ions

This means, that you have to find which of the choices is a solution that contains the same 0.300 M ion concentration.

2) 0.0800 M Na₂CO₃

• Na₂CO₃ (aq) → 2 Na⁺ + CO₃⁻

• 1 M Na₂CO₃ / 3 M ions = 0.0800M / x ⇒ x = 0.0267 M ions

This is not equal to 0.300 M, so this solution would not contain the same total concentration as a 0.100 M solution of K₂SO₄, and is not the right answer.

3)  0.100 M NaCl

• NaCl → Na⁺ + Cl⁻

• 1 M NaCl / 2 M ions = 0.100 M NaCl / x ⇒ x = 0.200 M ions

This is not equal to 0.300 M ion, so not a correct option.

4) 0.0750 M Na₃PO₄

• Na₃PO₄ → 3Na⁺ + PO₄³⁻

• 1 M Na₃PO₄ / 4 M ions = 0.0750 M Na₃PO₄ / x ⇒ x = 0.300 M ions

Hence, this ion concentration is equal to the ion concentration of a 0.100 M solution of K₂SO₄, and is the correct choice.

5)  0.0500 M NaOH

• NaOH → Na⁺ + OH⁻

• 1 M NaOH / 2 mol ions = 0.0500 M NaOH / x ⇒ x = 0.100 M ions

Not equal to 0.300 M, so wrong choice.

As the temperature of liquid increases, its vapor pressure increases. Therefore, option (2) is correct.

What is vapour pressure?

Vapour pressure can be defined as the pressure exerted by a vapor with its condensed phases in a closed system at a given temperature. The equilibrium vapor pressure is also served as an indicator of the rate of evaporation of a liquid.  

A material that has a high vapor pressure at normal temperatures is commonly referred to as a volatile material. The pressure exhibited by the molecules of the gas above a liquid surface is called vapor pressure.

The temperature and the vapor pressure of liquid are directly related to each other. If the temperature of the liquid increases, more gasmolecules have the energy to escape from the surface of the liquid.

Therefore, the vapor pressure increases with an increase in the temperature of the liquid.

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