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4 years ago

What is the concentration of a solution that contains 9 moles of solute in 3 liters of solution?

Chemistry

1 answer:

SVEN [57.7K]4 years ago

7 0

Answer:

Explanation:

mol solute / L soln. M = 5.50 mol / .600 L. M = 9.16 molar

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How many moles of H2O will be formed from the reaction of 80 g of

Roman55 [17]

Answer: 2 moles of $H_2O$ will be formed.

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} NaOH=\frac{80g}{40g/mol}=2moles$

The balanced chemical equation is:

$H_2SO_4+2NaOH\rightarrow Na_2SO_4+2H_2O$

According to stoichiometry :

2 moles of $NaOH$ give = 2 moles of $H_2O$

Thus 2 moles of $NaOH$ give = $\frac{2}{2}\times 2=2moles$ of $H_2O$

Thus 2 moles of $H_2O$ will be formed.

4 0

3 years ago

When two clear, colourless liquids are mixed together, a yellow precipitate is formed. This is an example of a

Flura [38]

Answer:

Combining the two clear colorless liquids is a chemical change.

Explanation:

Because a different solid substance is formed. Tell students that a precipitate is an insoluble solid that forms when two solutions are combined and react chemically. Insoluble means that the solid will not dissolve.

3 0

3 years ago

When light strikes a transparent material, most of the light is absorbed or reflected.

Monica [59]

When light strikes a transparent material, most of the light passes through it it doesn't absorb or reflect it

4 0

3 years ago

Read 2 more answers

How many moles are represented by 3.01 x10^24 oxygen atoms?

asambeis [7]

<h3>Answer:</h3>

5.00 mol O₂

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

<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>

Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.<u> </u>

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

3.01 × 10²⁴ atoms O₂

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

Avogadro's Number

<u>Step 3: Convert</u>

Set up: $\displaystyle 3.01 \cdot 10^{24} \ atoms \ O_2(\frac{1 \ mol \ O_2}{6.022 \cdot 10^{23} \ atoms \ O_2})$
Multiply/Divide: $\displaystyle 4.99834 \ mol \ O_2$