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3 years ago

What is the total number of atoms in CaCO3

Chemistry

2 answers:

nikitadnepr [17]3 years ago

7 0

Answer:

Here you go

Explanation:

Avogadro number is 6.023 x 10(23).

A mole of CaCO3 (calcium carbonate) has one mole (Avogadro number) of Ca atoms, one mole of C atoms and 3 moles of O atoms.

krek1111 [17]3 years ago

3 0

(I did look this up JUST to be sure!)

Explanation: A mole of CaCO3 (calcium carbonate) has one mole (Avogadro number) of Ca atoms, one mole of C atoms and 3 moles of O atoms.

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What is the limiting reactant and theoretical yield if 0.483 mol of Ti and 0.911 mol Clare used in this reaction: Ti + 2Cl2 → Ti

Mariana [72]

Answer : The limiting reactant is $Cl_2$ and the theoretical yield will be 86.45 grams.

Explanation : Given,

Moles of $Ti$ = 0.483 mole

Moles of $Cl_2$ = 0.911 mole

Molar mass of $TiCl_4$ = 190 g/mole

First we have to calculate the limiting and excess reagent.

The given balanced chemical reaction is,

$Ti+2Cl_2\rightarrow TiCl_4$

From the balanced reaction we conclude that

As, 2 moles of $Cl_2$ react with 1 mole of $Ti$

So, 0.911 moles of $Cl_2$ react with $\frac{0.911}{2}=0.455$ moles of $Ti$

From this we conclude that, $Ti$ is an excess reagent because the given moles are greater than the required moles and $Cl_2$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $TiCl_4$ .

As, 2 moles of $Cl_2$ react to give 1 moles of $TiCl_4$

So, 0.911 moles of $Cl_2$ react to give $\frac{0.911}{2}=0.455$ moles of $TiCl_4$

Now we have to calculate the mass of $TiCl_4$ .

$\text{Mass of }TiCl_4=\text{Moles of }TiCl_4\times \text{Molar mass of }TiCl_4$

$\text{Mass of }TiCl_4=(0.455mole)\times (190g/mole)=86.45g$

Therefore, the theoretical yield will be 86.45 grams.

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3 years ago

What determines the transition between different states of matter?

Scrat [10]

Answer:

Phase transition is when a substance changes from a solid, liquid, or gas state to a different state. Every element and substance can transition from one phase to another at a specific combination of temperature and pressure.

Explanation:

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3 years ago

How many F atoms are in this compound? 6MgF2 12 6 8 2

nevsk [136]

Answer:

5.0×1022 sa taas po yang 22

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3 years ago

Consider the following balanced equation for the following reaction:

castortr0y [4]

Answer:

47.47 g of CO₂ is the amount formed.

Explanation:

The reaction is:

2C₆H₅COOH(aq) + 15O₂(g) → 14CO₂(g) + 6H₂O(l)

Let's apply the formula for the percent yield

Percent yield of reaction = (Produced yield/Theoretical yield) . 100

First of all we convert the moles of CO₂ to mass: 1.30 mol . 44 g /1 mol = 57.2 g. So now, we replace:

(Produced yield / 57.2 g ). 100 = 83

Produced yield / 57.2 g = 83 / 100

Produced yield / 57.2 g = 0.83

Produced yield = 0.83 . 57.2g → 47.47 g of CO₂

8 0

3 years ago

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What can be added to an atom to cause a nonvalence electron in the atom to temporarily become a valence electron?

vazorg [7]

Answer:

What can be added to an atom to cause a nonvalence electron in the atom to temporarily become a valence electron is energy.

Explanation:

The normal state of the atoms, where all the electrons are occupying the lowest possible energy level, is called ground state.

The valence electrons are the electrons that occupy the outermost shell, this is the electrons in the highest main energy level (principal quantum number) of the atom.

So, a nonvalence electron occupies an orbital with less energy than what a valence electron does; in consequence, in order to a nonvalence electron jump from its lower energy level to the higher energy level of a valence electron, the former has to absorb (gain) energy.

This new state is called excited state and is temporary: the electron promoted to the higher energy level will emit the excess energy, in the form of light (photons), to come back to the lower energy level and so the atom return to the ground state.

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4 years ago

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