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2 years ago

What are some chemical formulas for compounds?

Chemistry

1 answer:

Galina-37 [17]2 years ago

4 0

Hello there!

First, we need to know what compounds are.
Compounds "are pure substances that are made up of two or more elements that are chemically combined in fixed mass ratios."

Now we need to understand what chemical formulas are.
The compounds have a chemical formula which tell us that
a) the elements that are present in the compound
b) the ratio of these elements in the compound

What are some chemical formulas for compounds?
Well, we start with water. The chemical formula for water is H2O

When we go back to the definition of compounds, it says it is when a pure substance that are made up two or more elements. So, whatever is a pure substance and it's made up of two elements. These elements are Hydrogen and Oxygen. And keep an mind that water is made up with metal plus non-metal.

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Here are one more chemical formulas for compounds
Sodium Chloride = NaCI

I included a picture that might help you too. (Credit to google image)

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Choose the element that IS NOT in the same period as Potassium.

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E. sodium is the answer

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3 years ago

A mixture of reactants and products for the reaction shown below is at

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If the volume of the container were increased to 4.0 L, more N₂ and H₂ would be produced (Option D)

<h3>What is chemical equilibrium? </h3>

This is simply defined as a state in a chemical system where there is no observable change in the properties of the system with time.

<h3>Principle of chemical equilibrium </h3>

A French scientist postulated a principle which helps us to understand a chemical system in equilibrium.

The principle states as follow:

If a an external constraint such as change in temperature, pressure or concentration is imposed on a system in equilibrium, the equilibrium will shift so as to neutralize the effect.

<h3>How to determine what will happen if the volume of the container is increased from 2 L to 4 L</h3>

From the principle given above, we can see that volume does not affect equilirium position.

However, from Boyle's law, we understood that pressure and volume are in invest relationship.

Thus, increasing volume simply means decreasing pressure.

A decrease in pressure will favors the side where there is an increase in volume.

Let us consider the equation from the question:

N₂(g) + 3H₂(g) <=> 2NH₃(g)

Volume of reactants = 1 + 3 = 4 L
Volume of products = 2 L

Thus, we can conclude that increasing the volume (i.e decreasing the pressure) of the reaction will favors the backward reaction, hence, more N₂ and H₂ would be produced.

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1 year ago

At a given temperature, the elementary reaction A − ⇀ ↽ − B , A↽−−⇀B, in the forward direction, is first order in A A with a rat

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Answer:

The equilibrium constant for the reversible reaction = 0.0164

Explanation:

At equilibrium the rate of forward reaction is equal to the rate of backwards reaction.

The reaction is given as

A ⇌ B

Rate of forward reaction is first order in [A] and the rate of backward reaction is also first order in [B]

The rate of forward reaction = |r₁| = k₁ [A]

The rate of backward reaction = |r₂| = k₂ [B]

(Taking only the magnitudes)

where k₁ and k₂ are the forward and backward rate constants respectively.

k₁ = 0.010 s⁻¹

k₂ = 0.0610 s⁻¹

|r₁| = 0.010 [A]

|r₂| = 0.016 [B]

At equilibrium, the rate of forward and backward reactions are equal

|r₁| = |r₂|

k₁ [A] = k₂ [B] (eqn 1)

Note that equilibrium constant, K, is given as

K = [B]/[A]

So, from eqn 1

k₁ [A] = k₂ [B]

[B]/[A] = (k₁/k₂) = (0.01/0.0610) = 0.0163934426 = 0.0164

K = [B]/[A] = (k₁/k₂) = 0.0164

Hope this Helps!!!

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2 years ago

What information does Jaime need to evaluate the accuracy of his calculation?

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Answer:

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3 years ago

Read 2 more answers

Gaseous methane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water. If 2.59 g of water is produc

max2010maxim [7]

<u>Answer:</u> The percent yield of the water is 31.98 %

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

<u>For methane:</u>

Given mass of methane = 6.58 g

Molar mass of methane = 16 g/mol

Putting values in equation 1, we get:

$\text{Moles of methane}=\frac{6.58g}{16g/mol}=0.411mol$

<u>For oxygen gas:</u>

Given mass of oxygen gas = 14.4 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{14.4g}{32g/mol}=0.45mol$

The chemical equation for the combustion of methane is:

$CH_4+2O_2\rightarrow CO_2+2H_2O$

By Stoichiometry of the reaction:

2 moles of oxygen gas reacts with 1 mole of methane

So, 0.45 moles of oxygen gas will react with = $\frac{1}{2}\times 0.45=0.225mol$ of methane

As, given amount of methane is more than the required amount. So, it is considered as an excess reagent.

Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction

2 moles of oxygen gas produces 2 moles of water

So, 0.45 moles of oxygen gas will produce = $\frac{2}{2}\times 0.45=0.45$ moles of water

Now, calculating the mass of water from equation 1, we get:

Molar mass of water = 18 g/mol

Moles of water = 0.45 moles

Putting values in equation 1, we get:

$0.45mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(0.45mol\times 18g/mol)=8.1g$

To calculate the percentage yield of water, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of water = 2.59 g

Theoretical yield of water = 8.1 g

Putting values in above equation, we get:

$\%\text{ yield of water}=\frac{2.59g}{8.1g}\times 100\\\\\% \text{yield of water}=31.98\%$

Hence, the percent yield of the water is 31.98 %

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2 years ago