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3 years ago

Can someone help me with that pls

Chemistry

2 answers:

kipiarov [429]3 years ago

6 0

Answer:

The one that's highlighted in blue is the answer

Rom4ik [11]3 years ago

3 0

Answer:

Explanation:

EVAPERATION --- is water falling back to the earth

CONDUNSATION -- Process where water vapor is cooled

RUNOFF ---- Process where the water that falls back down to earth runs over to lakes, river, and ocean

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Why does coal usually produce more soot than other fossil fuels when burned?

Elenna [48]

Answer and explanation;

Coal has aromatic hydrocarbons with high molar mass and has a high ratio of carbon to hydrogen. Burning coal produces more soot than burning other fossil fuels does because of it.

Fossil fuel mixtures of hydrocarbons that formed from the remains of plants or animals. Burning fossil fuels increases the amount of carbon dioxide in the atmosphere. This increase may affect temperatures, amounts of rain and sea levels worldwide. Some sulfur and nitrogen are in fossil fuels, and air contains nitrogen.

6 0

3 years ago

Tony thinks the unknown is KI while Steve thinks the unknown is LiCL. Who is correct? Support your choice with evidence/reaction

qaws [65]

Answer:

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4 0

3 years ago

How many grams of KCl 03 are needed to produce 6.75 Liters of O2 gas measured at 1.3 atm pressure and 298 K?

Nina [5.8K]

11.48-gram of $KCl0_3$ are needed to produce 6.75 Liters of $O_2$ gas measured at 1.3 atm pressure and 298 K

<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).

First, calculate the moles of the gas using the gas law,

PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= 1.3 atm

V= 6.75 Liters

n=?

R= $0.082057338 \;L \;atm \;K^{-1}mol^{-1}$

T=298 K

Putting value in the given equation:

$\frac{PV}{RT}=n$

$n= \frac{1.3 \;atm\; X \;6.75 \;L}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 298}$

Moles = 0.3588 moles

Now,

$Moles = \frac{mass}{molar \;mass}$

$0.3588 moles = \frac{mass}{32}$

Mass= 11.48 gram

Hence, 11.48-gram of $KCl0_3$ are needed to produce 6.75 Liters of $O_2$ gas measured at 1.3 atm pressure and 298 K

Learn more about the ideal gas here:

brainly.com/question/27691721

#SPJ1

3 0

2 years ago

Ammonia (NH3) can be produced by the reaction of hydrogen gas with nitrogen gas:

sp2606 [1]

B) 40%
The balanced equation indicates that for every 3 moles of H2 used, 2 moles of NH3 will be produced. So the reaction if it had 100% yield would produce (2.00 / 3) * 2 = 1.333333333 moles of NH3. But only 0.54 moles were produced. So the percent yield is 0.54 / 1.3333 = 0.405 = 40.5%. This is a close enough match to option "b" to be considered correct.

3 0

3 years ago

Read 2 more answers

A mixture of 14.0 grams of H2, 84.0 grams of N2, and 64.0 grams of O2 are placed in a flask. The partial pressure of the O2 is 7

Hitman42 [59]

Answer:

$P_{tot}=465.27torr$

Explanation:

Hello there!

In this case, according to the given information, it will be possible for us to use the Dalton's law, in order to solve this problem. However, we first need to calculate the mole fraction of oxygen by firstly calculating the moles of each gas:

$n_{H_2}=\frac{14.0g}{2.02g/mol} =6.93mol\\\\n_{N_2}=\frac{84.0g}{28.02g/mol}=3.00mol\\\\n_{O_2}=\frac{64.0}{16.00g/mol} =2.00mol$

Next, we calculate such mole fraction as follows:

$x_{O_2}=\frac{2}{6.93+3+2} =0.168$

Then, given the following equation:

$P_{O_2}=P_{tot}*x_{O_2}$

So we solve for the total pressure as follows:

$P_{tot}=\frac{P_{O_2}}{x_{O_2}} \\\\P_{tot}=\frac{78.00torr}{0.168} \\\\P_{tot}=465.27torr$

Regards!

6 0

3 years ago