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3 years ago

What would be the result if Earth's unique atmosphere did not exist?

Chemistry

2 answers:

Goshia [24]3 years ago

6 0

Answer:

D) Life will no longer be possible

Explanation:

Odyssey ware

egoroff_w [7]3 years ago

5 0

Then the earth would most likely not be able to support life. Our earth would be similar to mars. In that it might have supported life. It the thin atmosphere would over all be unable to sustain more complex species. The earth would also be much colder because the green house effect is what maintains our relatively warm atmosphere.

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Write the formula for potassium nitride? (show work) CAN SOMEONE PLEASE HELP?

ohaa [14]

Answer:

It should b KNO3

Explanation:

one Potassium (K) and three Nitrite (NO3)

8 0

2 years ago

How many molecules of sodium nitrate are produced when 40 g of sodium azide, NaN3, react with oxygen?

quester [9]

NaN 3 + AgNO 3 AgN 3 + NaNO 3

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2 years ago

Ow many coulombs of charge are needed to produce 35.2 mol of solid zinc?

Natasha2012 [34]

Answer: Zn(2+) + 2e(-) -------> Zn 1 mole of Zn is deposited by 2F of electricity ... so 48.9 mole of Zn will be deposited by 48.9 X 2F = 97.8 F of electricity... as 1F = 96500 C so 97.8 F = 97.8 X 96500 = 9437700 C of electricity...

8 0

3 years ago

Read 2 more answers

When nitrogen dioxide (NO2) from car exhaust combines with water in the air, it forms nitric acid (HNO3), which causes acid rain

yKpoI14uk [10]

Answer:

For a: The number of molecules of nitrogen dioxide is $4.52\times 10^{23}$

For b: The mass of nitric acid formed is 54.81 grams

For c: The mass of nitric acid formed is 206 grams

Explanation:

The given chemical reaction follows:

$3NO_2(g)+H_2O(l)\rightarrow 2HNO_3(aq.)+NO(g)$

For a:

By Stoichiometry of the reaction:

1 mole of water reacts with 3 moles of nitrogen dioxide

So, 0.250 moles of water will react with $\frac{3}{1}\times 0.250=0.75mol$ of nitrogen dioxide

According to mole concept:

1 mole of a compound contains $6.022\times 10^{23}$ number of molecules.

So, 0.75 moles of nitrogen dioxide will contain $0.75\times 6.022\times 10^{23}=4.52\times 10^{23}$ number of molecules

Hence, the number of molecules of nitrogen dioxide is $4.52\times 10^{23}$

For b:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of nitrogen dioxide = 60.0 g

Molar mass of nitrogen dioxide = 46 g/mol

Putting values in equation 1, we get:

$\text{Moles of nitrogen dioxide}=\frac{60.0g}{46g/mol}=1.304mol$

By Stoichiometry of the reaction:

3 moles of nitrogen dioxide produces 2 mole of nitric acid

So, 1.304 moles of nitrogen dioxide will produce = $\frac{2}{3}\times 1.304=0.870$ moles of nitric acid

Now, calculating the mass of nitric acid from equation 1, we get:

Molar mass of nitric acid = 63 g/mol

Moles of nitric acid = 0.870 moles

Putting values in equation 1, we get:

$0.870mol=\frac{\text{Mass of nitric acid}}{63g/mol}\\\\\text{Mass of nitric acid}=(0.870mol\times 63g/mol)=54.81g$

Hence, the mass of nitric acid formed is 54.81 grams

For c:

For nitrogen dioxide:

Given mass of nitrogen dioxide = 225 g

Molar mass of nitrogen dioxide = 46 g/mol

Putting values in equation 1, we get:

$\text{Moles of nitrogen dioxide}=\frac{225g}{46g/mol}=4.90mol$

For water:

Given mass of water = 55.2 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

$\text{Moles of water}=\frac{55.2g}{18g/mol}=3.06mol$

By Stoichiometry of the reaction:

3 moles of nitrogen dioxide reacts with 1 mole of water

So, 4.90 moles of nitrogen dioxide will react with = $\frac{1}{3}\times 4.90=1.63mol$ of water

As, given amount of water is more than the required amount. So, it is considered as an excess reagent.

Thus, nitrogen dioxide is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

3 mole of nitrogen dioxide produces 2 moles of nitric acid

So, 4.90 moles of nitrogen dioxide will produce $\frac{2}{3}\times 4.90=3.27mol$ of nitric acid

Now, calculating the mass of nitric acid from equation 1, we get:

Molar mass of nitric acid = 63 g/mol

Moles of nitric acid = 3.27 moles

Putting values in equation 1, we get:

$3.27mol=\frac{\text{Mass of nitric acid}}{63g/mol}\\\\\text{Mass of nitric acid}=(3.27mol\times 63g/mol)=206g$

Hence, the mass of nitric acid formed is 206 grams

7 0

2 years ago

What type of atom is hydrogen with an atomic mass of 1 and 2 electrons

Charra [1.4K]

Answer:

This would be the hydride ion where H gains an electron from a metal such as Na

Explanation:

7 0

3 years ago