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Brut [27]
2 years ago
7

Calculate the pressure of 2.50 Liters of a gas at 25.0oC if it has a volume of 4.50 Liters at

Chemistry
1 answer:
MariettaO [177]2 years ago
4 0

Answer:

P_2 =0.51  atm

Explanation:

Given that:

Volume (V1) = 2.50 L

Temperature (T1) = 298 K

Volume (V2) = 4.50 L

at standard temperature and pressure;

Pressure (P1) = 1 atm

Temperature (T2) = 273 K

Pressure P2 = ??

Using combined gas law:

\dfrac{P_1V_1}{T_1} = \dfrac{P_2V_2}{T_2} \\ \\ \dfrac{1 *2.5}{298} = \dfrac{P_2*4.5}{273}

0.008389261745 \times 273 = 4.5P_2

P_2 =\dfrac{0.008389261745 \times 273 }{4.5}

P_2 =0.51 \ atm

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andreev551 [17]

Answer:

Sln

n=m/mr

n=25/100

n=0.25mole of Caco3

Malality =number of moles/volume (divided by number of moles both sides)

volume =Malality /number of moles

v=0.125/0.25

v=0.500L

I hope this help

5 0
2 years ago
Why is it the principle about the relationship between mass and volume always true of substance, but not always true of mixtures
Xelga [282]

Answer:

For pure substances, the mass and volume will always be the same or will always change the same way because all substance are the same throughout.

While for mixtures, you can have varying amount of each component therefore mass and volume will not change the same way for substances

7 0
1 year ago
The particles of a gas inside a balloon are experiencing an increase in the average kinetic energy and the number of collisions
Sever21 [200]

Answer:

1. Higher gas pressure inside the balloon.

Explanation:

An increase in the average kinetic energy and the number of collisions represents increases on gas temperature and pressure inside the ballon. Hence, the answer is 1.

6 0
3 years ago
Limestone is formed from:
Semmy [17]

sand silt and clay but also has large amounts of Carbonate. NOT carbonite.

5 0
2 years ago
Read 2 more answers
A 5.024 mg sample of an unknown organic molecule containing carbon, hydrogen, and nitrogen only was burned and yielded 13.90 mg
Dafna1 [17]

Answer:

C8H17N

Explanation:

Mass of the unknown compound = 5.024 mg

Mass of CO2 = 13.90 mg

Mass of H2O = 6.048 mg

Next, we shall determine the mass of carbon, hydrogen and nitrogen present in the compound. This is illustrated below:

For carbon, C:

Molar mass of CO2 = 12 + (2x16) = 44g/mol

Mass of C = 12/44 x 13.90 = 3.791 mg

For hydrogen, H:

Molar mass of H2O = (2x1) + 16 = 18g/mol

Mass of H = 2/18 x 6.048 = 0.672 mg

For nitrogen, N:

Mass N = mass of unknown – (mass of C + mass of H)

Mass of N = 5.024 – (3.791 + 0.672)

Mass of N = 0.561 mg

Now, we can obtain the empirical formula for the compound as follow:

C = 3.791 mg

H = 0.672 mg

N = 0.561 mg

Divide each by their molar mass

C = 3.791 / 12 = 0.316

H = 0.672 / 1 = 0.672

N = 0.561 / 14 = 0.040

Divide by the smallest

C = 0.316 / 0.04 = 8

H = 0.672 / 0.04 = 17

N = 0.040 / 0.04 = 1

Therefore, the empirical formula for the compound is C8H17N

8 0
3 years ago
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