Answer:
Molecular formula = P₄O₁₀
Explanation:
Given data:
Empirical formula of compound = P₂O₅
Molar mass of compound = 426 g/mol
Molecular formula = ?
Solution:
Molecular formula:
Molecular formula = n (empirical formula)
n = molar mass of compound / empirical formula mass
Empirical formula mass= P₂O₅ = 283.89 g/mol
n = 426 g/mol / 283.89 g/mol
n = 2
Molecular formula = n (empirical formula)
Molecular formula = 2 (P₂O₅ )
Molecular formula = P₄O₁₀
Answer:
When atoms are formed or broken.
Explanation:
The substances that go into a chemical reaction are called the reactants, and the substances produced at the end of the reaction are known as the products.
Answer:
H2O
Explanation:
Water is both an Arrhenius acid and base.
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Molar mass
<h3><u>Explanation</u>;</h3>
- Stoichiometry involves the study of quantitative relationships between the amounts of reactants used and products formed by a chemical reaction.
- A conversion factor is a ratio of coefficients found in a balanced reaction, which can be used to inter-convert the amount of products and reactants.
- Molar ratios, or conversion factors, identify the number of moles of each reactant needed to form a certain number of moles of each product.
Answer:
97.2g
Explanation:
Step 1:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
Ca(OH)2 + 2HCl —> CaCl2 + 2H2O
Step 2:
Determination of the number of mole of water (H2O) to produce from the reaction.
This is illustrated below:
From the balanced equation above,
1 mole of Ca(OH)2 produced 2 moles of H2O.
Therefore, 2.70moles of Ca(OH)2 will produce = 2.7 x 2 = 5.4 moles of H2O.
Step 3:
Converting 5.4 moles of H2O to grams. This is illustrated below:
Number of mole of H2O = 5.4 moles
Molar Mass of H2O = (2x1) + 16 = 2 + 16 = 18g/mol
Mass of H2O =?
Mass = number of mole x molar Mass
Mass of H2O = 5.4 x 18
Mass of H2O = 97.2g
Therefore, 97.2g of water is produced from the reaction.
