Answer:
The molar mass of Barium Oxide, BaO is 153.33g/mol.
Explanation:
The molar mass of a compound is defined as the sum of the relative atomic mass of the atoms which forms the chemical compound.
The atomic mass of Barium Ba = 137.33
Atomic mass of Oxygen O = 16.00
Adding the respective atomic mass together we have;
BaO = 137.33 + 16.00
BaO=153.33g/mol.
So therefore, the molar mass of Barium Oxide BaO is 153.33g/mol.
Answer:
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Answer:
46.71g
Explanation:
First, we'll begin by calculating the number of mole of KNO3 present in the solution. This is illustrated below below:
Data obtained from the question:
Molarity = 2.50 M
Volume = 185 mL = 185/1000 = 0.185L
Mole =?
Molarity = mole /Volume
Mole = Molarity x Volume
Mole = 2.5 x 0.185
Mole = 0.4625 mole
Now we can obtain the mass of KNO3 as follow:
Molar Mass of KNO3 = 39 + 14 + (16x3) = 39 + 14 + 48 = 101g/mol
Number of mole of KNO3 = 0.4625 mole
Mass of KNO3 =?
Mass = number of mole x molar Mass
Mass of KNO3 = 0.4625 x 101
Mass of KNO3 = 46.71g
Answer:
Kc = 2.145 × 10⁻⁸¹
Explanation:
Let's consider the following reaction:
O₂(g) ⇄ 2O(g)
The standard Gibbs free energy for the reaction (ΔG°) can be calculated using the following expression:
ΔG° = Σnp. ΔG°f(p) - Σnp. ΔG°f(p)
where,
ni are the moles of products and reactants
ΔG°f(p) are the standard Gibbs free energy of formation of products and reactants
In this case,
ΔG° = 2 × ΔG°f(O) - 1 × ΔG°f(O₂)
ΔG° = 2 × 230.1 kJ/mol - 1 × 0 kJ/mol
ΔG° = 460.2 kJ/mol
With this information, we can calculate the equilibrium constant (Kc) using the following expression:
1: viewing any chemical reaction in a laboratory
2: dangerous to look at when it burns & used in photography, fireworks, and flares
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