Answer:
2. Isotope, one of two or more species of atoms of a chemical element with the same atomic number and position in the periodic table and nearly identical chemical behavior but with different atomic masses and physical properties. Every chemical element has one or more isotopes.
3. Since the vast majority of an atom's mass is found its protons and neutrons, subtracting the number of protons (i.e. the atomic number) from the atomic mass will give you the calculated number of neutrons in the atom. In our example, this is: 14 (atomic mass) – 6 (number of protons) = 8 (number of neutrons).
Explanation: Try rewording the questions when looking it up. Hope this helps
Answer: 19kpa
Explanation:
The total pressure of a mixture of gases is the sum of the partial pressure exacted by the individual gases.
P total = P X + P Y
From the question above:
P total = P .nitrogen + P. oxygen
123.5kpa = 104.5kpa + P. Oxygen
P. Oxygen = 123.5kpa - 104.5kpa
= 19kpa
Answer:
3.75 moles
Explanation:
The chemical equation is 2CH₃OH + 3O₂ -> 2CO₂ + 4H₂O
2 moles of CH₃OH are burned by 3 moles of O₂
For 2.5 moles of CH₃OH are burned by x moles of O₂
Let's solve for x :
2*x=2.5*3 => 2*x=7.5 => x=3.75 moles of O₂ are needed to burn 2.5 moles of CH₃OH
The moles of oxygen required to burn Butane is 6 moles.
<h3>What is a Combustion Reaction?</h3>
A reaction in which fuel gets oxidised by an oxidising agent producing a large amount of heat is called a combustion reaction.
In this question
Butane is burnt with oxygen
Molar mass of C₄H₁₀ = (12.0×4 + 1.0×10) g/mol = 58.0 g/mol
Molar mass of O₂ = 16.0×2 g/mol = 32.0 g/mol
Balanced equation for the reaction:
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O
Mole ratio C₄H₁₀ : O₂ = 2 : 13
The given mass = 54grams
moles = 54/58 = 0.93 moles
The mole of oxygen required =
0.93/ x = 2/13
0.93*13/2 = x
x = 6.045 moles
Therefore 6 moles of oxygen are required to burn Butane.
To know more about Combustion Reaction
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The answer should be neutralization
