Answer:
8.31 × 10⁻²² kJ
Explanation:
Step 1: Given data
Energy required to remove one mole of electrons from the atoms at the surface of a solid metal: 500 kJ/mol e⁻
Step 2: Calculate how much energy does it take to remove a single electron from an atom at the surface of this solid metal
We will use Avogadro's number: there are 6.02 × 10²³ electrons in 1 mole of electrons.
500 kJ/mol e⁻ × 1 mol e⁻/6.02 × 10²³ e⁻ = 8.31 × 10⁻²² kJ/e⁻
Answer:
im also BOREDDDDDDDDDDDD.....
Answer:
2.90 x 10⁻¹¹moldm⁻³
Explanation:
Given parameters:
[H⁺] = 3.5 x 10⁻⁴mol/dm³
Unknown
[OH⁻] = ?
Solution;
The ionic product of water can be used to solve this problem. It has been experimentally determined to be 1 x 10⁻¹⁴mol² dm⁻⁶
[H⁺] [OH⁻] = 1 x 10⁻¹⁴
Therefore;
[OH⁻] = 
= 
= 0.29 x 10⁻¹⁰moldm⁻³
= 2.90 x 10⁻¹¹moldm⁻³
P * V = n R T
<span>1 * 2.50 = n * 0.082 * 273 = 2. 50 / ( 0.082 * 273 ) = 0.11 mol </span>
<span>mass = mole number * molecular mass </span>
<span>mass = 0.11 * ( 16 * 2 ) = 3.52 g </span>
Answer:
Two
Explanation:
I believe your unbalanced equation should be
H₂O₂ + I₂ ⟶ IO₃⁻
The half-reactions and the overall reaction are:
5 × [H₂O₂ + 2H⁺ +2e⁻ ⟶ 2H₂O]
1 × <u>[ I₂ + 6H₂O ⟶ 2IO₃⁻ + 12H⁺ + 10e⁻]
</u>
5H₂O₂ + I₂ ⟶ 2IO₃⁻ + 2H⁺ + 4H₂O
The reaction needs two hydrogen ions for balancing.
