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3 years ago

The expulsion of an electron from an atomic nucleus is called _______ decay.

1 answer:

8 0

The expulsion of an electron from an atomic nucleus is called β⁻<span> decay.

</span>β decay is a type of radiation and it consists of two parts as β⁻ decay and β⁺ decay.

β⁻ decay is a conversion of neutron into a proton by emission of an electron.
when an element undergoes a β⁻ decay, the daughter nucleus will have the same number of mass but the number of protons will be increased by 1 and number of neutron will be decreased by 1.

β⁺ decay is a conversion of proton into a neutron by emitting a positron. Then daughter nucleus will have same number of mass but proton number will be decreased by 1 and neutron number will be increased by 1.

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Consider the following equation: SiO2 (s) + 3C (graphite) --> SiC (s) + 2CO (g) ΔH rxn = 624.6 kJ / mol rxn. Using the follow

DerKrebs [107]

<u>Answer:</u> The enthalpy of the formation of $SiC(s)$ is coming out to be -65.3 kJ/mol

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as $\Delta H^o$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f_{(product)}]-\sum [n\times \Delta H^o_f_{(reactant)}]$

For the given chemical reaction:

$SiO_2(s)+3C\text{ (graphite)}(s)\rightarrow SiC(s)+2CO(g)$

The equation for the enthalpy change of the above reaction is:

$\Delta H^o_{rxn}=[(1\times \Delta H^o_f_{(SiC(s))})+(2\times \Delta H^o_f_{(CO(g))})]-[(1\times \Delta H^o_f_{(SiO_2(s))})+(3\times \Delta H^o_f_{(C(s))})]$

We are given:

$\Delta H^o_f_{(CO(g))}=-110.5kJ/mol\\\Delta H^o_f_{(SiO_2(s))}=-910.9kJ/mol\\\Delta H^o_f_{(C(s))}=0kJ/mol\\\Delta H^o_{rxn}=624.6kJ$

Putting values in above equation, we get:

$624.6=[(1\times \Delta H^o_f_{(SiC(s))})+(2\times (-110.5))]-[(1\times (-910.9))+(3\times (0))]\\\\\Delta H^o_f_{(SiC(s))}=-65.3kJ/mol$

Hence, the enthalpy of the formation of $SiC(s)$ is coming out to be -65.3 kJ/mol.

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4 years ago

What is electrolysis <br><br><br> What is alternating current?

Mashutka [201]

The meaning of electrolysis-chemical decomposition produced by passing an electric current through a liquid or solution containing ions. Alternating- occur in turn repeatedly.

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3 years ago

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C4H10+ 02 → CO2 +H2O <br> balance the equation

rewona [7]

Answer:

C4H10 + 502 -> CO2 + 5H20

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3 years ago

If normal rainfall has a pH of 6.2 and acid rain has a pH of 2.8, how much greater is the hydrogen ion concentration of the acid

Ymorist [56]

Taking into account the definition of pH, the hydrogen ion concentration of the acid rain is 1.58×10⁻³ greater compared to normal rainfall.

<h3>Definition of pH</h3>

pH is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance.

The pH is defined as the negative base 10 logarithm of the activity of hydrogen ions, that is, the concentration of hydrogen ions or H₃O⁺:

pH= - log [H⁺]= - log [H₃O⁺]

<h3>Normal rainfall</h3>

Normal rainfall has a pH of 6.2. Replacing in the definition of pH:

6.2= - log [H⁺]

Solving:

[H⁺]= 10⁻⁶ ²

Acid rain has a pH of 2.8. Replacing in the definition of pH:

2.8= - log [H⁺]

Solving:

[H⁺]= 10⁻² ⁸

<h3>Hydrogen ion concentration difference of acid rain compared to normal rain.</h3>

To know how much greater is the hydrogen ion concentration of the acid rain compared to normal rainfall, you must do the subtraction between both concentrations:

1.58×10⁻³ - 6.31×10⁻⁷= 1.58×10⁻³

It is practically equal to the concentration of hydrogen ions in acid rain because its concentration is much higher than the concentration in normal rainfall.

In summary, the hydrogen ion concentration of the acid rain is 1.58×10⁻³ greater compared to normal rainfall.

Learn more about pH:

brainly.com/question/12200689

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2 years ago

How is firelight produced

malfutka [58]

Firelighting<span> is the process by which a </span>fire<span> can be started artificially. </span>

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3 years ago

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