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aleksandr82 [10.1K]
3 years ago
5

Using words, explain all steps of dimensional analysis when converting 6.7 hectometers to meters. You must explain the set up of

the problem and give your final answer.
A minimum of 4 complete sentences are

Chemistry
1 answer:
Anettt [7]3 years ago
7 0

Answer:

\large \boxed{\text{670 m}}

Explanation:

Dimensional analysis uses the fact that any number can be multiplied by one without changing its value.

You want to convert hectometres to metres, so you multiply the hectometres by a conversion factor that equals one.

For example, you know that hecto  means "× 10², so  

1 hm = 100 m

If we divide each side by 1 hm, we get 1 = 100 m/1 hm.

If we divide each side by 100 m, we get 1 hm/100 m = 1.

So, we can use either (100 m/1 hm) or (1 hm/100 m) as a conversion factor, because each fraction equals one.

We choose the former, because it has the desired units on top.

The calculation becomes

\text{Distance} = \text{6.7 hm} \times \dfrac{\text{100 m}}{\text{1 hm}} = \textbf{670 m}\\\\\text{6.7 hm} =\, $\large \boxed{\textbf{670 m}}$}

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3. Given 20g of Barium Hydroxide, how many grams of
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The number of grams of ammonium nitrate (NH₄NO₃) it would take for all the barium hydroxide to react is 18.7g

First, we will write the balanced chemical equation for the reaction

The balanced chemical equation for the reaction is

Ba(OH)₂ + 2NH₄NO₃ → 2NH₄OH + Ba(NO₃)₂

This means, 1 mole of barium hydroxide is required to react with 2 moles of ammonium nitrate

Now, we will calculate the number of moles of barium hydroxide present.

Mass of barium hydroxide (Ba(OH)₂) = 20 g

Using the formula

Number\ of\ moles = \frac{Mass}{Molar\ mass}

Molar mass of Ba(OH)₂ = 171.34 g/mol

∴ Number of moles of Ba(OH)₂ present =\frac{20}{171.34}

Number of moles of Ba(OH)₂ present = 0.116727 mole

Now,

Since 1 mole of barium hydroxide is required to react with 2 moles of ammonium nitrate

Then,

0.116727 mole of barium hydroxide will react with 2 × 0.116727 mole of ammonium nitrate

2 × 0.116727 = 0.233454 mole

∴ Number of moles of NH₄NO₃ required is 0.233454 mole

Now, for the mass of ammonium nitrate (NH₄NO₃) required

From the formula

Mass = Number of moles × Molar mass

Molar mass of NH₄NO₃ = 80.043 g/mol

∴ Mass of NH₄NO₃ required = 0.233454 × 80.043

Mass of NH₄NO₃ required = 18.68636 g

Mass of NH₄NO₃ required ≅ 18.7g

Hence, the number of grams of ammonium nitrate (NH₄NO₃) it would take for all the barium hydroxide to react is 18.7g

Learn more on determining mass of reactant required here: brainly.com/question/11232389

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