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2 years ago

Question 1-8

Chemistry

1 answer:

JulijaS [17]2 years ago

3 0

If 28.0 grams of a gas occupies 22.4 liters at STP, the gas could be carbon monoxide, CO

<h3>Ideal gas </h3>

We understood from the ideal gas equation that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure (STP)

<h3>How to determine the identity of the gas</h3>

To determine the identity of the gas, we shall determine the mass of 1 mole of each gas. This can be obtained as

For C₂H₂

1 mole of C₂H₂ = (12×2) + (2×1) = 26 g

For C₂H₆

1 mole of C₂H₆ = (12×2) + (6×1) = 30 g

For CO₂

1 mole of CO₂ = 12 + (16×2) = 44 g

For CO

I mole of CO = 12 + 16 = 28 g

From the above illustrations, we can see that 1 mole of CO is equivalent to 28 g.

Thus, the correct answer to the question is CO

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What is the scientific notation of 36000x10 ex.10?

Vedmedyk [2.9K]

Answer:

3.6 times 10^4

Explanation:

Scientific notation is between 1-9. So, we move 36000 to 4 decimal places. SO it would be 3.6 times 10^4. Scientific Notation always has the base of 10 . Enjoy :)

5 0

4 years ago

When dinitrogen pentaoxide, a white solid, is heated, it decomposes to produce nitrogen dioxide gas and

AysviL [449]

9.5314 L is the volume of nitrogen dioxide formed at 103.25 kPa and 22.75 °C.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Given data:

Oxygen produced - 1.618 gram

Decomposition of $N_2O_5$ takes place.

Find - Amount of $NO_2$ produced.

The decomposition reaction is as follows -

$2N_2O_5$ --> $4NO_2 + O_2$

Moles of $O_2$ gas = $\frac{1.6}{16}$ =0.1 moles.

1 mole of $O_2$ is produced from 2 moles of dinitrogen pentoxide

0.1 mole of $O_2$ will be produced from = 0.2 moles.

Now, 2 moles of dinitrogen pentoxide produce 4 moles of $NO_2$

$NO_2$ produced will be - 0.4 moles.

Weight of $NO_2$ produced - 0.4 X 46

Weight of $NO_2$ produced - 18.4 gram

Thus, grams of $NO_2$ produced are 18.4

Now calculate the volume of $NO_2$

Given data are:

P=103.25 kPa =1.01899827 atm

T= 22.75 °C +273 = 295.75 K

n=0.4 moles

V=?

R= 0.0821 liter·atm/mol·K

Putting the value in PV=nRT

V = $\frac{nRT}{P}$

V = $\frac{0.4 \;moles \;X \;0.0821\; liter\;atm/\;mol \;K X \;295.75 \;K}{1.01899827 atm}$

V= 9.5314 L

Hence, 9.5314 L is the volume of nitrogen dioxide formed at 103.25 kPa and 22.75 °C.

Learn more about the ideal gas equation here:

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8 0

2 years ago

In the waves lab, you changed ______ to see how it would affect wave speed.

jasenka [17]

Hi there!

I believe the answer is transversal or transverse.

Have a nice night!
~Brooke

4 0

3 years ago

Read 2 more answers

What is a physical change that could not easily be reversed?

mylen [45]

Answer:

the answer is number 1

Explanation:

because when you make toast you burn it you toast it and there is no way to undo that.

8 0

3 years ago

What is the complete set of quantum numbers for the fifth electron added to a hydrogen ion?

N76 [4]

1s2 2s2 2p1

fifth electron is in 2p orbital

so answer is 2 2 -1 -1/2 , or 2 2 -1 1/2

*1/2 and -1/2 are spins, so they are interchangeable when writing the first electron in the ml

8 0

3 years ago