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3 years ago

5

The molecular weight of a compound is the sum of the atomic weights of all atoms in the molecule. What is the molecular mass of

acetaminophen, (C8H9NO2), the active ingredient in Tylenol?

1 answer:

larisa [96]3 years ago

4 0

Answer:

abcdefghijklmnopqrstuvwxyznendjdkdkjchnsskd

dhdjsjsjjd

Explanation:

djjdjdjsdkkxjsk

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Which pair could be genetic clones?<br><br> look at the photo

noname [10]

Answer:

cow female

Explanation:

7 0

3 years ago

What is the mass of 2.16 moles of sulfur dioxide (SO2)?

Luda [366]

<h3>Answer:</h3>

138 g SO₂

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

[Given] 2.16 moles SO₂

[Solve] grams (mass) SO₂

<u>Step 2: Identify Conversions</u>

[PT] Molar Mass of S - 32.07 g/mol

[PT] Molar Mass of O - 16.00 g/mol

Molar Mass of SO₂ - 32.07 + 2(16.00) = 64.07 g/mol

<u>Step 3: Convert</u>

[DA] Set up: $\displaystyle 2.16 \ mol \ SO_2(\frac{64.07 \ g \ SO_2}{1 \ mol \ SO_2})$
[DA] Multiply/Divide [Cancel out units]: $\displaystyle 138.391 \ g \ SO_2$

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

138.391 g SO₂ ≈ 138 g SO₂

6 0

3 years ago

How many atoms are in 1 mole of Carbon tetrachloride?

lesantik [10]

Answer:

There is one carbon atom in every carbon tetrachloride molecule, which means that there is an equal number of carbon atoms to carbon tetrachloride molecules. 5.089 x 1022 atoms of C.

Explanation:

Hope this helped, Have a Wonderful Day!!

3 0

3 years ago

Which of these statements is correct? a. Particles in a suspension will settle out if left undisturbed. b. A solution is heterog

tatuchka [14]

Blood. It is discrete cells in saline solutuion. The cells are free to move thru the plasma, or you wouldn't have blood flow, or oxygenation, and you would die. Blood is defined as liquid, not jello.

The other three are things not normally associated--water will fall from the sky as rain, for example, but is held in suspension in fog. Same with the salad oil in mayo. O.J. can be a suspension; easily separated by a filter, Or a colloid--depends if the pulp, if Any, is held in suspension or not. Usually, pulp will settle to the bottom, making that sample of Orange juice a suspension. At different temperatures, it acts differently. But, so does Fog. A colloid is something that normally shouldn't be as some of its molecules are too dense to normally "float" in suspension. Colloid means "glue".

4 0

3 years ago

What mass of iron(II) oxide must be used in the reaction given by the equation below to release 44.7 kJ? 6FeO(s) + O2(g) => 2

zavuch27 [327]

<u>Answer:</u> The mass of iron (II) oxide that must be used in the reaction is 30.37

<u>Explanation:</u>

The given chemical reaction follows:

$6FeO(s)+O_2(g)\rightarrow 2Fe_3O_4(s);\Delta H^o=-635kJ$

By Stoichiometry of the reaction:

When 635 kJ of energy is released, 6 moles of iron (II) oxide is reacted.

So, when 44.7 kJ of energy is released, $\frac{6}{635}\times 44.7=0.423mol$ of iron (II) oxide is reacted.

Now, calculating the mass of iron (II) oxide by using the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Moles of iron (II) oxide = 0.423 moles

Molar mass of iron (II) oxide = 71.8 g/mol

Putting values in above equation, we get:

$0.423mol=\frac{\text{Mass of FeO}}{71.8g/mol}\\\\\text{Mass of FeO}=(0.423mol\times 71.8g/mol)=30.37g$

Hence, the mass of iron (II) oxide that must be used in the reaction is 30.37

7 0

4 years ago