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3 years ago

What is the symbol for inches?

Chemistry

2 answers:

Harman [31]3 years ago

6 0

My bad. I was incorrect the answer above is right

Angelina_Jolie [31]3 years ago

4 0

' is for ft.
" is for inches.

Example, someone is 5"4'

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A sample of CaCO3 (molar mass 100. g) was reported as being 30. percent Ca. Assuming no calcium was present in any impurities, c

natka813 [3]

Answer:

Approximately 75%.

Explanation:

Look up the relative atomic mass of Ca on a modern periodic table:

Ca: 40.078.

There are one mole of Ca atoms in each mole of CaCO₃ formula unit.

The mass of one mole of CaCO₃ is the same as the molar mass of this compound: $\rm 100\; g$ .
The mass of one mole of Ca atoms is (numerically) the same as the relative atomic mass of this element: $\rm 40.078\; g$ .

Calculate the mass ratio of Ca in a pure sample of CaCO₃:

$\displaystyle \frac{m(\mathrm{Ca})}{m\left(\mathrm{CaCO_3}\right)} = \frac{40.078}{100} \approx \frac{2}{5}$ .

Let the mass of the sample be 100 g. This sample of CaCO₃ contains 30% Ca by mass. In that 100 grams of this sample, there would be $\rm 30 \% \times 100\; g = 30\; g$ of Ca atoms. Assuming that the impurity does not contain any Ca. In other words, all these Ca atoms belong to CaCO₃. Apply the ratio $\displaystyle \frac{m(\mathrm{Ca})}{m\left(\mathrm{CaCO_3}\right)} \approx \frac{2}{5}$ :

$\begin{aligned} m\left(\mathrm{CaCO_3}\right) &= m(\mathrm{Ca})\left/\frac{m(\mathrm{Ca})}{m\left(\mathrm{CaCO_3}\right)}\right. \cr &\approx 30\; \rm g \left/ \frac{2}{5}\right. \cr &= 75\; \rm g \end{aligned}$ .

In other words, by these assumptions, 100 grams of this sample would contain 75 grams of CaCO₃. The percentage mass of CaCO₃ in this sample would thus be equal to:

$\displaystyle 100\%\times \frac{m\left(\mathrm{CaCO_3}\right)}{m(\text{sample})} = \frac{75}{100} = 75\%$ .

3 0

3 years ago

Another term for natural radioactive decay into another element is

Musya8 [376]

Answer:

The process of unstable (or radioactive) atoms becomes stable by emitting radiation. This event over time is called radioactive decay. Alpha decay results in the loss of two protons and two neutrons from the nucleus

6 0

3 years ago

Read 2 more answers

Iron, an important component of the steel used in the construction of buildings, bridges, and railroads, combines with oxygen to

vladimir2022 [97]

I don't understand, what you want?

3 0

4 years ago

What statement is incorrect about this oxidation-reduction reaction? 2 SO2(g) + O2(g) → 2 SO3(g) What statement is incorrect abo

Leno4ka [110]

Answer:

The incorrect statement is: SO₂ gains electrons

Explanation:

A chemical reaction that involves the simultaneous transfer of electrons between two chemical species, is known as the redox reaction.

Given chemical reaction: 2SO₂(g) + O₂(g) → 2SO₃(g)

In this redox reaction, S is present in +4 oxidation state in SO₂ and +6 oxidation state SO₃. Whereas, O is present in 0 oxidation state in O₂ and -2 oxidation state in SO₃.

Therefore, SO₂ loses electrons and thus gets oxidized. Whereas, O₂ gains electrons and thus gets reduced.

In this reaction, SO₂ is the reducing agent and O₂ is the oxidizing agent.

6 0

3 years ago

The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of

Basile [38]

Answer:

1.57 mol NaN₃

Explanation:

2 NaN₃ (s) → 2 Na (s) + 3 N₂ (g)

First we use PV=nRT to calculate the number of N₂ moles that need to be produced:

P = 1.07 atm

V = 53.4 L

n = ?

R = 0.082 atm·L·mol⁻¹·K⁻¹

T = 23.7 °C ⇒ 23.7 + 273.16 = 296.86 K

Inputing the data:

1.07 atm * 53.4 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 296.86

And solving for n:

n = 2.35 mol N₂

Finally we convert N₂ moles into NaN₃ moles, using the stoichiometric coefficients of the balanced reaction:

2.35 mol N₂ * $\frac{2molNaN_3}{3molN_2}$ = 1.57 mol NaN₃

4 0

3 years ago