Answers are:
1) The balanced oxidation half reaction: 2I⁻(aq) → I₂(s) + 2e⁻.
Iodine is oxidized (lost electrons) from -1 to neutral charge (0).
2) The balanced reduction half-reaction: 2H₂O(l) + 2e⁻ → H₂(g) + 2OH⁻.
Hydrogen is reduced (gain electrons) from +1 to neutral charge.
3) The oxidation <span>reaction takes place at the anode.</span>
Answer:
0.055g/mL
Explanation:
Data obtained from the question include:
Molar Mass of the gass sample = 71g/mol
Volume of the gas sample = 1300 mL
Density =?
The density of a substance is simply mass per unit volume. It is represented mathematically as:
Density = Mass /volume.
With the above equation, we can easily obtain the density of sample of gas as illustrated below:
Density = 71g / 1300 mL
Density = 0.055g/mL
Therefore, the density of the gas sample is 0.055g/mL
Water is a polar molecule, meaning the covalent bonds in it share electrons unequally. They spend more time around the oxygen, making it positive and the hydrogens negative. This helps water stick to surfaces, a property called adhesion. The hydrogens of one molecule are also attracted to the oxygens of another. This is called cohesion, and it helps water form droplets
Holy I'm not that smart lol but I'll get back to you
Answer:
80.27%
Explanation:
Let's consider the following balanced equation.
2 Fe³⁺(aq) + Sn²⁺(aq) ⇒ 2Fe²⁺(aq) + Sn⁴⁺(aq)
First, we have to calculate the moles of Sn²⁺ that react.
We also know the following relations:
- According to the balanced equation, 1 mole of Sn²⁺ reacts with 2 moles of Fe³⁺.
- 1 mole of Fe³⁺ is oxidized from 1 mole of Fe.
- The molar mass of Fe is 55.84 g/mol.
Then, for 1.348 × 10⁻3 moles of Sn²⁺:
If there are 0.1505 g of Fe in a 0.1875 g sample, the mass percentage of Fe is:
