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4 years ago

12

Matter is made up of tiny particles that are too small to be seen with the naked eye. these tiny particles are known as _______.

2 answers:

VladimirAG [237]4 years ago

8 0

Matter is made up of particles too small to be seen with the naked eye called atoms

MArishka [77]4 years ago

4 0

Explanation:

Any substance which occupies some space and has some mass is known as matter.

Every matter is made up of tiny particles which are known as atoms. Any matter can either have same atoms or with different atoms.

Thus, we can conclude that matter is made up of tiny particles that are too small to be seen with the naked eye. These tiny particles are known as atoms.

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________ is the study of matter and the energy that causes matter to combine, break apart and recombine in everything living and

Kipish [7]

Answer: Emperical formula

Explanation:

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3 years ago

How do you use the periodic table to determine the mass of 4 moles of oxygen? Explain your process for getting the answer. Use s

Nitella [24]

Answer:

read back through your lesson and get the formula

Explanation:

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3 years ago

Read 2 more answers

How many moles of magnesium is 1.25 x 1023 atoms of magnesium?

andrew-mc [135]

The moles of magnesium in 1.25 x 1023 are 20.8 mol.

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4 years ago

What is the mass of oxygen in 300 grams of carbonic acid (H2CO3)

DENIUS [597]

mass of carbonic acid = 300g

molar mass of H2CO3 = 2H + C + 3 O

= 2 x 1.008+ 12.01 + 3 x 16

= 62.03g/mol

moles of H2CO3 = mass/Molar mass

= 300/62.03

= 4.8364 moles

1 mole H2CO3 has 3 moles Oxygen

4.8364 moles H2CO3 contains

= 3 x 4.8364 moles Oxygen = 14.509 moles Oxygen

moles = mass/Molar mass

mass of oxygen = moles x Molar mass of Oxygen

= 14.509 x 16

= 232.15g Oxygen

mass of oxygen in 300g of carbonic acid(H2CO3) = 232.15g

7 0

3 years ago

A sample of gas in a 14.6 L flexible container is at 25.0oC and 1.00atm. What is the volume of the sample when heated to 220.0oC

inn [45]

Answer: 24.1 L

Explanation:

To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

where,

$V_1\text{ and }T_1$ are the initial volume and temperature of the gas.

$V_2\text{ and }T_2$ are the final volume and temperature of the gas.

We are given:

$V_1=14.6L\\T_1=25.0^oC=(25+273)K=298K\\V_2=?\\T_2=220.0^0C=(220+273)K=493K$

Putting values in above equation, we get:

$\frac{14.6}{298K}=\frac{V_2}{493}\\\\V_2=24.1L$

Thus the volume of the sample when heated to 220.0oC and the pressure is constant is 24.1 L

7 0

3 years ago