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3 years ago

Perform the following operation

Chemistry

1 answer:

Yanka [14]3 years ago

3 0

Taking into account the scientific notation, the result of the sum is 10.84300×10³.

<u><em>Scientific notation</em></u>

First, remember that scientific notation is a quick way to represent a number using powers of base ten.

The numbers are written as a product:

a×10ⁿ

where:

a is a real number greater than or equal to 1 and less than 10, to which a decimal point is added after the first digit if it is a non-integer number.
n is an integer, which is called an exponent or an order of magnitude. Represents the number of times the comma is shifted. It is always an integer, positive if it is shifted to the left, negative if it is shifted to the right.

<u><em>Sum in scientific notation</em></u>

You want to add two numbers in scientific notation. It should be noted that when the numbers to be added do not have the same base 10 exponent, the base 10 power with the highest exponent must be found. In this case, the highest exponent is 3.

Then all the values are expressed as a function of the base 10 exponent with the highest exponent. In this case: 9.7300×10²= 0.97300×10³

Taking the quantities to the same exponent, all you have to do is add what was previously called the number "a". In this case:

0.97300×10³ + 9.8700×10³= (0.97300+ 9.8700)×10³= 10.84300×10³

Finally, the result of the sum is 10.84300×10³.

Learn more:

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3 years ago

In a calorimeter, a 1.0 g sample of magnesium is burned to form mgo. in doing so, 25.5 kj of energy are released. what is the mo

Artemon [7]

The molar enthalpy of combustion in kj/mol of magnesium is 620 kj/mol, Option D is the correct answer.

<h3>What is enthalpy of Combustion ?</h3>

The energy released when a fuel is oxidized by an oxidizing agent is called enthalpy of Combustion.

It is given that

a 1.0 g sample of magnesium is burned to form MgO. in doing so, 25.5 kj of energy are released.

Molecular weight of Magnesium = 24.35g

24.35 g makes 1 mole of Mg

1g = 1/24.35

For 0.04 moles 25.5 kJ is released

for 1 mole 25.5 *1/.04

= 620 kj/mol

Therefore the molar enthalpy of combustion in kj/mol of magnesium is 620 kj/mol.

To know more about enthalpy of combustion

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2 years ago

Atrazine is an herbicide widely used for corn and is a common groundwater pollutant in the corn-producing regions of the United

riadik2000 [5.3K]

Answer:

0.94

Explanation:

Let's assume that the total sample of the soil is 1 cm³; which has a porosity of 0.4 cm³; then the original sample of the soil will be 0.6 cm³

The mass of the soil particles in 1 cm³ of soil + water = 0.75 g

The fraction of the total atrazine can be calculated by the expression;

Total atrazine = $C_w(\frac{g}{mL})*V_w(mL)+C_{(soil)}(\frac{g}{soil})*M_{(soil)}(gsoil)$

Also; $C_{(soil)}(\frac{g}{soil})= K_{oc}(\frac{mL}{gOC})*f_{oc} (\frac{gOC}{gsoil})*C_w(\frac{g}{mL})$

NOTE THAT: $K_{oc}( \frac{mL}{gOC})=K_{oc}\frac{L}{kgOC}$

Total atrazine can now be calculated as:

$C_w*0.4+K_{oc}f_{oc}C_w*0.75$ = $\frac{C_{soil}*M_{soil}}{Total atrazine}$

$=\frac{K_{oc}f_{oc}C_w*M_{soil}}{C_w*0.4+K_{oc}f_{oc}C_w*0.75} = \frac{0.75*K_{oc}f_{oc}}{0.4+K_{oc}f_{oc}*0.75}$

$= \frac{10^{2.52}*0.025*0.75}{0.4+10^{2.52}*0.025*0.75}$

= 0.94

Thus,the fraction of total atrazine that will be adsorbed to the soil = 0.94.

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4 years ago