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2 years ago

HELP ME OUT MY LOVELY CHEMISTRY CHADS I WILL GIVE YOU A KISS

Chemistry

1 answer:

vitfil [10]2 years ago

6 0

Answer:

300K.

Explanation:

The following data were obtained from the question:

Initial volume (V1) = 300L

Initial temperature (T1) = 200K

Final volume (V2) = 450L

Final temperature (T2) =..?

Since the pressure is constant, the gas is obeying Charles' law.

Using the Charles' law equation, we can obtain the new temperature of the gas as follow:

V1/T1 = V2/T2

300/200 = 450/T2

Cross multiply to express in linear form

300 x T2 = 200 x 450

Divide both side by 300

T2 = (200 x 450)/ 300

T2 = 300K

Therefore, the new temperature of the gas is 300K.

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What fraction of the gas phase molecules initially present for 1.0 atm in the chamber are present at 1.0×10−10 torr?

vivado [14]

The fraction of gas phase molecules is calculated by the division of final pressure to the initial pressure.

Fraction = $\frac{P_{final}}{P_{initial}}$ (1)

Here, initial pressure = 1.0 atm

final pressure = $1.0\times 10^{-10} torr$

First, convert torr into atm

1 atm = 760 torr

final pressure = $\frac{1.0\times 10^{-10}}{760}$

= $1.316\times 10^{-13}atm$

Now, put the value of initial and final pressure in formula (1)

Fraction = $\frac{1.316\times 10^{-13}atm}{1.0 atm}$

= $1.316\times 10^{-13}$

Thus, fraction of the gas phase molecules = $1.316\times 10^{-13}$ $\simeq 1.3\times 10^{-13}$

7 0

3 years ago

The pressure at the top of Mount Everest is 33.7 kPa. Is this greater or less than 0.25<br> atm?

Fantom [35]

Answer:1 atm = 101,325 Pa

So, you convert 33.7 KPa to Pa and divide by 101,325, as follows:

3.7 KPa (1 x 10^3Pa / 1 KPa) (1 atm / 101,325 Pa) = .33 atm

As you can see 33.7 KPa, which is equal to .33 atm, is greater than 0.25.

Explanation: why didnt you just look this up jeez

7 0

2 years ago

5. A Dumas bulb is filled with chlorine gas at the ambient pressure and is found to contain 7.1 g of chlorine when the temperatu

kati45 [8]

Answer:

a. The original temperature of the gas is 2743K.

b. 20atm.

Explanation:

a. As a result of the gas laws, you can know that the temperature is inversely proportional to moles of a gas when pressure and volume remains constant. The equation could be:

T₁n₁ = T₂n₂

<em>Where T is absolute temperature and n amount of gas at 1, initial state and 2, final states.</em>

<em />

<em>Replacing with values of the problem:</em>

T₁n₁ = T₂n₂

X*7.1g = (X+300)*6.4g

7.1X = 6.4X + 1920

0.7X = 1920

X = 2743K

<h3>The original temperature of the gas is 2743K</h3><h3 />

b. Using general gas law:

PV = nRT

<em>Where P is pressure (Our unknown)</em>

<em>V is volume = 2.24L</em>

<em>n are moles of gas (7.1g / 35.45g/mol = 0.20 moles)</em>

R is gas constant = 0.082atmL/molK

And T is absolute temperature (2743K)

P*2.24L = 0.20mol*0.082atmL/molK*2743K

<em />

7 0

2 years ago

For the equation 2H₃PO₄ + 3Ca ⇒ 3H₂ + Ca₃(PO₄)₂ suppose you had 27.4 grams of H₃PO₄?

Darya [45]

Answer:

Explanation:

Given 2H₃PO₄ + 3Ca ⇒ 3H₂ + Ca₃(PO₄)₂

27.4g

=(27.4g/98g/mol)

= 0.280 mole H₃PO₄ used

Ca Used:

Rxn Ratio H₃PO₄ : Ca => 2:3

∴ moles Ca used = 3/2(0.280) mole Ca =0.420 mole Ca

grams Ca used = 0.420 mole Ca x 40 g/mole = 16.8 grams Ca used

Grams H₂ Produced:

Rxn Ratio H₃PO₄ : H₂ => 2:3 => moles H₂ produced = 3/2(0.28 mole H₂) = 0.420 mole H₂ = (0.420 mole H₂ x 2.02 g/mole) = 0.8484 grams H₂(g) Produced.

Moles Ca₃(PO₄)₂ Produced:

FWt Ca₃(PO₄)₂ = 310 g/mole

Rxn Ratio H₃PO₄ : Ca₃(PO₄)₂ => 2:1

∴moles Ca₃(PO₄)₂ Produced = 1/2(moles H₃PO₄ used)

= 1/2(0.28 mole) = 0.14 mole Ca₃(PO₄)₂

If you want grams Ca₃(PO₄)₂, multiply moles Ca₃(PO₄)₂ by formula weight.

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2 years ago

You have performed some tests on a piece of an unknown solid element. Here are the results. Melting Point = 98oC Shiny appearanc

tangare [24]

Answer:

it can be both actually both a non metal and a metal

5 0

1 year ago