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4 years ago

What is the proper name for MgSO4 7H2O?

Chemistry

2 answers:

Tems11 [23]4 years ago

8 0

Answer: Option (A) is the correct answer.

Explanation:

When two different atoms combine together in similar composition they result in the formation of a compound.

And when a chemical formula include water molecules then it is represented by a dot followed by compound formula and then number of water molecules along with water formula are written.

For example, $MgSO_{4}.7H_{2}O$ is a compound that has seven water molecules.

According to naming nomenclature, "hepta" will represent seven.

Thus, we can conclude that name of $MgSO_{4}.7H_{2}O$ is Magnesium sulfate heptahydrate.

lukranit [14]4 years ago

7 0

A. magnesium sulfate heptahydrate
that is what it stands for

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he mass defect of the helium nucleus ⁴He₂ is 0.030377 u

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Rutherford’s major achievements : brainly.com/question/1552732

Unit of radius of an atom : brainly.com/question/1968819

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Answer details

Grade: College

Subject: Physics

Chapter: Nuclear Physics

Keywords: Mass , Defect , Nucleon , Number , Atomic , Proton , Electron , Neutron

4 0

3 years ago

Consider the balanced equation for the following reaction:

Zanzabum

Answer: The amount of carbon dioxide formed in the reaction is 5.663 grams

Explanation:

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

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

Given mass of oxygen gas = 8 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{8g}{32g/mol}=0.25mol$

For the given chemical equation:

$7O_2(g)+2C_2H_6(g)\rightarrow 4CO_2(g)+6H_2O(l)$

By Stoichiometry of the reaction:

7 moles of oxygen gas produces 4 moles of carbon dioxide

So, 0.25 moles of oxygen gas will produce = $\frac{4}{7}\times 0.25=0.143mol$ of carbon dioxide

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

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 0.143 moles

Putting values in equation 1, we get:

$0.143mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(0.143mol\times 44g/mol)=6.292g$

To calculate the experimental yield of carbon dioxide, we use the equation:

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

Percentage yield of carbon dioxide = 90 %

Theoretical yield of carbon dioxide = 6.292 g

Putting values in above equation, we get:

$90=\frac{\text{Experimental yield of carbon dioxide}}{6.292g}\times 100\\\\\text{Experimental yield of carbon dioxide}=\frac{90\times 6.292}{100}=5.663g$

Hence, the amount of carbon dioxide formed in the reaction is 5.663 grams

7 0

3 years ago

If we know this is a second-order reaction, what is the rate law?

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Answer:

The rate is a mathematical relationship obtained by comparing reaction rate with reactant concentrations.

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3 years ago