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3 years ago

What's the Molar Mass of O2? O 16.0 g/mole o 32.0 g/mole 1.0 g/mole O 2.0 g/mole

Chemistry

2 answers:

stiks02 [169]3 years ago

5 0

............:.................................

Elza [17]3 years ago

5 0

32.0 g/mol! Take the atomic mass off of the periodic table (16) and multiply by 2 since there are two oxygen atoms. So your answer is 32.0 g/mol.

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What are 2 indications that a chemical change has occurred?

irakobra [83]

Answer: The color has changed or the formation of light and heat. Also, the temprature will change as well.

Explanation:

8 0

3 years ago

difference between an Argon atom with a mass number of 38 (Ar-38) and another Argon atom with a mass number of 45 (Ar-45)?

Kay [80]

The difference between Argon-38 and Argon - 45 is the number of neurons in their nuclei.

<h3>What is Isotope?</h3>

Isotopes are two or more types of atoms of the same element that have the same atomic number but differs in mass numbers due to different numbers of neutrons in their nuclei.

Argon atom with a mass number of 38 (Ar-38) - number of neutrons = 20

Argon atom with a mass number of 45 (Ar-45) - number of neutrons = 27

Thus, the difference between Argon-38 and Argon - 45 is the number of neurons in their nuclei.

Learn more about isotopes here: brainly.com/question/364529
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8 0

2 years ago

Question 1(Multiple Choice Worth 4 points)

zubka84 [21]

<u>Answer </u>

Answer 1 : 28.9 g of CO is needed.

Answer 2 : Six moles of $H_{2}O$ over Nine moles of $O_{2}$

Answer 3 : Four over two fraction can be used for the mole ratio to determine the mass of Fe from a known mass of $Fe_{2}O_{3}$ .

Answer 4 : Mass of $O_{2}$ = (150 × 3 × 31.998) ÷ (232.29 × 1) grams

Answer 5 : 8.4 moles of sodium cyanide (NaCN) would be needed.

<u>Solution </u>

Solution 1 : Given,

Given mass of $Fe_{2}O_{3}$ = 55 g

Molar mass of $Fe_{2}O_{3}$ = 159.69 g/mole

Molar mass of CO = 28.01 g/mole

Moles of $Fe_{2}O_{3}$ = $\frac{\text{ Given mass of } Fe_{2}O_{3}}{\text{ Molar mass of } Fe_{2}O_{3}}$ = $\frac{55 g}{159.69 g/mole}$ = 0.344 moles

Balanced chemical reaction is,

$Fe_{2}O_{3}(s)+3CO(g)\rightarrow 2Fe(s)+3CO_{2}(g)$

From the given reaction, we conclude that

1 mole of $Fe_{2}O_{3}$ gives → 3 moles of CO

0.344 moles of $Fe_{2}O_{3}$ gives → 3 × 0.344 moles of CO

= 1.032 moles

Mass of CO = Number of moles of CO × Molar mass of CO

= 1.032 × 28.01

= 28.90 g

Solution 2 : The balanced chemical reaction is,

$2C_{3}H_{6}+9O_{2}\rightarrow 6CO_{2}+6H_{2}O$

From the given reaction, we conclude that the Six moles of $H_{2}O$ over Nine moles of $O_{2}$ is the correct option.

Solution 3 : The balanced chemical reaction is,

$4Fe+3O_{2}\rightarrow 2Fe_{2}O_{3}$

From the given balanced reaction, we conclude that Four over two fraction can be used for the mole ratio to determine the mass of Fe from a known mass of $Fe_{2}O_{3}$ .

Solution 4 : Given,

Given mass of $Zn(ClO_{3})_{2}$ = 150 g

Molar mass of $Zn(ClO_{3})_{2}$ = 232.29 g/mole

Molar mass of $O_{2}$ = 31.998 g/mole

Moles of $Zn(ClO_{3})_{2}$ = $\frac{\text{ Given mass of }Zn(ClO_{3})_{2} }{\text{ Molar mass of } Zn(ClO_{3})_{2}}$ = $(\frac{150\times 1}{232.29})moles$