Answer:
0.9852 moles of CaO
Explanation:
Reaction equation for the decomposition of CaCO₃:
CaCO₃ → CaO + CO₂
The question asks how many moles of CaO form when 98.60g of CaCO₃ decompose.
We can see from the reaction equation that for every mol of CaCO₃, one mol of CaO will be produced (molar ratio 1:1)
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So first we need to calculate how many moles are the 98.60g of CaCO₃:
Molar Mass of CaCO₃ = molar mass Ca + molar mass C + 3 * molar mass O
= 40.078 + 12.011 + 3 * 15.999 = 100.086 g/mol
Moles of CaCO₃ = mass CaCO₃ / molar mass CaCO₃
Moles of CaCO₃ = 98.60 g / 100.086 g/mol = 0.9852 moles CaCO₃
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As we said before for every mol of CaCO₃, one mol of CaO is produced.
So the decomposition of 0.9852 moles of CaCO₃ will produce 0.9852 moles of CaO.
Hey I think it is going to be 0986 moles. Cuz we can see that no. of moles of CaCO3 which will decompose is equivalent to the no. of CaO . Now it's just the matter of finding the no. of moles of CaCO3 .
no.of moles=mass /relative molecular mass
Propyne has one triple bond between the two carbons HC≡C-CH₃ while heptene has one double bond between two carbons in the chain of the seven carbon atoms.
The 1st step for the IUPAC name is to select the longest, most substituted carbon chain with a functional substituent chosen. Then the use of the primary suffix indicates the degree of saturation in the structure such as 'ane' or 'ene.
The 'ane' suffix is used for a singlebond while 'ene' suffix is used for a doublebond and 'yne' is used for triple bonds.
Then the identification of the secondary suffix indicates the functional substituent in the molecule which depends on the number of times the same functional substituent is repeated such as di, tri, tetra, etc.
In the structure of heptene, the double bond can be present between any two adjacent carbons. If the double bond is present at the third and 4th carbon then it can be named 3-heptene.
Learn more about IUPAC nomenclature, here:
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An ion differs from an atom in that it has a net electrical charge, either positive or negative, due to the loss or gain of electrons.
An ion differs from an atom in that it has a net electrical charge. This charge is either positive or negative, resulting from the loss or gain of electrons by the atom. When an atom loses electrons, it becomes positively charged and forms a cation. On the other hand, when an atom gains electrons, it becomes negatively charged and forms an anion.
For example, let's consider sodium (Na) and chloride (Cl) atoms. Sodium has 11 protons and 11 electrons, making it neutral. However, when it loses an electron, it becomes a sodium ion (Na+), which now has 11 protons and 10 electrons, giving it a +1 charge. Chloride, on the other hand, has 17 protons and 17 electrons, making it neutral. But when it gains an electron, it becomes a chloride ion (Cl-), which now has 17 protons and 18 electrons, giving it a -1 charge.
So, while an atom is electrically neutral, an ion has a charge due to the loss or gain of electrons.
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Answer:
MgO.
Explanation:
charges of both satisfy one another (balanced) -- producing a compound MgO.
An oxidation reaction involves the loss of electrons or an increase in the oxidation state of an element. Options B, C, and D represent oxidation reactions, while option A does not.
Let's analyze the given options:
A. AuCl₄⁻ → AuCl₂⁻
In this reaction, the gold atom goes from a +3 oxidation state (AuCl₄⁻) to a +1 oxidation state (AuCl₂⁻). This means the gold atom gains two electrons, indicating a reduction rather than oxidation. Therefore, option A is not an oxidation reaction.
B. Mn⁷⁺ → Mn²⁺
In this reaction, the manganese atom goes from a +7 oxidation state to a +2 oxidation state. This indicates a decrease in the oxidation state, which means the manganese atom gains electrons. Therefore, option B represents an oxidation reaction.
C. Co³⁺ → Co²⁺
In this reaction, the cobalt atom goes from a +3 oxidation state to a +2 oxidation state. Similar to option B, this indicates a decrease in the oxidation state, representing an oxidation reaction.
D. Cl₂ → ClO₃⁻
In this reaction, the chlorine molecule (Cl₂) is converted to a chlorate ion (ClO₃⁻). Here, the chlorine atom undergoes an increase in oxidation state, changing from an oxidation state of 0 in Cl₂ to an oxidation state of +5 in ClO₃⁻. This indicates the loss of electrons by chlorine, making option D an oxidation reaction.
Therefore, options B, C, and D represent oxidation reactions, while option A does not.
Learn more about oxidation reaction from the link given below.
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