his is the chemical formula for chromium(III) nitrate: . Calculate the mass percent of oxygen in chromium(III) nitrate. Round yo

1) reacting hydrochloric acid with nickel:

Balanced molecular equation: Ni(s) + 2HCl(aq) → NiCl₂(aq) + H₂(g).

Ionic equation: Ni(s) + 2H⁺(aq) + 2Cl⁻(aq) → Ni²⁺(aq) + 2Cl⁻(aq) + H₂(g).

Net ionic equation: Ni(s) + 2H⁺(aq) → Ni²⁺(aq) + H₂(g).

In this reaction, nickel undergoes oxidation, changing from an oxidation state of 0 to +2, while hydrogen is reduced from +1 to 0 (H₂).

2) reacting sulfuric acid with iron:

Balanced molecular equation: Fe(s) + H₂SO₄(aq) → FeSO₄(aq) + H₂(g).

Ionic equation: Fe(s) + 2H⁺(aq) + SO₄²⁻(aq) → Fe²⁺(aq) + SO₄²⁻(aq) + H₂(g).

Net ionic equation: Fe(s) + 2H⁺(aq) → Fe²⁺(aq) + H₂(g).

In this scenario, iron is oxidized from an oxidation state of 0 to +2, while hydrogen experiences reduction from +1 to 0 (H₂).

3) hydrobromic acid reacting with magnesium:

Balanced molecular equation: Mg(s) + 2HBr(aq) → MgBr₂(aq) + H₂(g).

Ionic equation: Mg(s) + 2H⁺(aq) + 2Br⁻(aq) → Mg²⁺(aq) + 2Br⁻(aq) + H₂(g).

Net ionic equation: Mg(s) + 2H⁺(aq) → Mg²⁺(aq) + H₂(g).

This reaction sees magnesium oxidized from 0 to +2, and hydrogen reduced from +1 to 0 (H₂).

4) acetic acid reacting with zinc:

Balanced molecular equation: Zn(s) + 2CH₃COOH(aq) → (CH₃COO)₂Zn(aq) + H₂(g).

Ionic equation: Zn(s) + 2H⁺(aq) + 2CH₃COO⁻(aq) → Zn²⁺(aq) + 2CH₃COO⁻(aq) + H₂(g).

Net ionic equation: Zn(s) + 2H⁺(aq) → Zn²⁺(aq) + H₂(g).

Here, zinc gets oxidized from 0 to +2 (Zn²⁺), while hydrogen is reduced from +1 to 0 (H₂).

Answer:

• A. Which element, X or Z, has a higher molar mass?

Explanation:

Heating the original compounds intensely to remove all oxygen causes chemical decomposition reactions:

• 2XClO₃ (solid) → 2XCl + 3O₂ (gas)

• 2ZClO₃ (solid) → 2ZCl + 3O₂ (gas)

By measuring the initial mass of each sample and the mass remaining after heating, the student can compute the oxygen gas mass released:

• Mass of oxygen released = initial sample mass minus residue mass

Using this oxygen mass, she can calculate how many moles of oxygen were present in each sample:

• Moles of oxygen = oxygen mass (g) divided by molar mass of oxygen

Next, the moles of the original sample are determined:

• Each mole of XClO₃ or ZClO₃ has 3 moles of oxygen atoms.

So, dividing the moles of oxygen released by 3 gives the moles of the sample.

Applying the formula molar mass = mass / moles, the student finds the molar masses of XClO₃ and ZClO₃.

Thus, this data allows answering question A: Which of X or Z has the higher molar mass?

The issue with your setup is that the surface where you placed the drop is contaminated or dirty, preventing it from being wetted by the solution. To fix this, thoroughly clean the surface before applying the drop.

Answer:

yes

Explanation:

yes

Answer:

8 protons, 8 electrons, and 10 neutrons

Explanation: