, a crystal structure with a short symmetrical hydrogen bond.
<h3>What is Classical bonding?</h3>
Classical models of the chemical bond. By classical, we mean models that do not take into account the quantum behaviour of small particles, notably the electron. These models generally assume that electrons and ions behave as point charges which attract and repel according to the laws of electrostatics.
Sodium dihydrogen phosphate is a derivative composed of glycerol derivatives formed by reacting mono and diglycerides that are derived from edible sources with phosphorus pentoxide followed by neutralization with sodium carbonate.
Bonding in
, a crystal structure with a short symmetrical hydrogen bond. Sodium dihydrogen phosphate () is monoclinic, space group P2,/c, with a= 6.808 (2), b= 13.491 (3), c=7.331 (2)/~, fl=92.88 (3) ; Z=8.
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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:
Answer: orientation , energy , frequency
Explanation:
According to the collision theory , the number of collisions that take place per unit volume of the reaction mixture is called collision frequency. The effective collisions are ones which result into the formation of products.
Effective collisions depends on the following two factors:-
1. Orientation factor: The colliding molecules must have proper orientation at the time of collision to result into formation of products.
2. Energy factor: For collision to be effective, the colliding molecules must have energy more than a particular value called as threshold energy.
Answer:
5.00 mol Mg
10.0 mol Cl
40.0 mol O
Explanation:
Step 1: Given data
Moles of Mg(ClO₄)₂: 5.00 mol
Step 2: Calculate the number of moles of Mg
The molar ratio of Mg(ClO₄)₂ to Mg is 1:1.
5.00 mol Mg(ClO₄)₂ × 1 mol Mg/1 mol Mg(ClO₄)₂ = 5.00 mol Mg
Step 3: Calculate the number of moles of Cl
The molar ratio of Mg(ClO₄)₂ to Cl is 1:2.
5.00 mol Mg(ClO₄)₂ × 2 mol Cl/1 mol Mg(ClO₄)₂ = 10.0 mol Cl
Step 4: Calculate the number of moles of O
The molar ratio of Mg(ClO₄)₂ to Cl is 1:8.
5.00 mol Mg(ClO₄)₂ × 8 mol O/1 mol Mg(ClO₄)₂ = 40.0 mol O
Answer:
solid
Explanation:
It is called an amorphous solid because it lacks the ordered molecular structure of true solids, and yet its irregular structure is too rigid for it to qualify as a liquid.
