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3 years ago

14

According to _________ Law, the volume of a fixed amount of gas at a constant pressure varies directly with its absolute tempera

ture.
A) Avogadro's
B) Boyle's
C) Charles's
D) Combined

1 answer:

Dmitrij [34]3 years ago

7 0

The answer would be Boyle’s law

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En la reacción I2(g) + Br2(g) « 2 IBr(g), Keq = 280 a 150°C. Suponga que se permite que 0.500 mol de IBr en un matraz de 1.00 L

love history [14]

Answer:

P IBr: 15.454atm

I₂: 0.923 atm

P Br₂: 0.923atm

Explanation:

Basados en la reacción:

I₂(g) + Br₂(g) ⇄ 2 IBr(g)

La constante de equilibrio, Keq, es definida como:

$Keq = \frac{P_{IBr}^2}{P_{I_2}P_{Br_2}}$

<em>Se cumple la relación de Keq = 280 cuando las presiones están en equilibrio</em>

Usando PV = nRT, la presión inicial de IBr es:

P = nRT / V; 0.500mol*0.082atmL/molK*423.15K / 1.00L = <em>17.3 atm</em>

<em />

Siendo las presiones en equilibrio:

P IBr: 17.3 - 2X

P I₂: X

P Br₂: X

<em>Donde X representa el avance de reacción.</em>

Remplazando en Keq:

280 = (17.3 - 2X)² / X²

280X² = 4X² - 69.2X + 299.29

0 = -276X² - 69.2X + 299.29

<em>Resolviendo para X:</em>

X = -1.174 → Solución falsa. No existen presiones negativas

X = 0.923 → Solución real

Así, las presiones parciales en equilibrio de cada compuesto son:

P IBr: 17.3 - 2X = <em>15.454atm</em>

P I₂: X =<em> 0.923atm</em>

P Br₂: X = <em>0.923atm</em>

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3 years ago

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A student hypothesized that the green color of plant leaves is related to exposure to sunlight and tested this hypothesis by pla

kkurt [141]

The hypothesis is that
the green coloration of plants is related to sunlight exposure of leaves
The hypothesis is tested by keeping a dark green plant inside a dark closet
The result is that the green coloration faded
The conclusion must be that exposure to sunlight affects the green color of the plants

8 0

3 years ago

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A 50 L cylinder is filled with argon gas to a pressure of 10130.0 kPa at 300°C. How many moles of argon gas does the cylinder co

Vlad1618 [11]

To answer this question, we will use the general gas law which states that:
PV = nRT where:
P is the pressure of the gas = <span>10130.0 kPa
</span>V is the volume of the gas = 50 liters
n is the number of moles that we want to calculate
R is the gas constant = <span>8.314 L∙kPa/K∙mol
T is the temperature = 300+273 = 573 degree kelvin

Substitute with the givens in the equation to get the number of moles as follows:
</span><span>10130 * 50 = n * 8.314 * 573
506500 = 4763.922 n
n = </span>506500 / 4763.922
n = 106.3199 moles

7 0

3 years ago

How much heat is released when 24.8 g of ch4 is burned in excess oxygen gas?

balu736 [363]

The given question is incomplete. The complete question is:

How much heat is produced when 24.8 g of $CH_4$ is burned in excess oxygen gas

Given: $CH _4
+2O_2\rightarrow CO_2+2H_2O$ ΔH= −802 kJ.

Answer: 1243.1 kJ

Explanation:

Heat of combustion is the amount of heat released on complete combustion of 1 mole of substance.

Given :

Amount of heat released on combustion of 1 mole of methane = 802 kJ kJ/mol

According to avogadro's law, 1 mole of every substance occupies 22.4 L at NTP, weighs equal to the molecular mass and contains avogadro's number $6.023\times 10^{23}$ of particles.

1 mole of $CH_4$ weighs = 16 g

Thus we can say:

16 g of $CH_4$ on combustion releases heat = 802 kJ

Thus 24.8 g of $CH_4$ on combustion releases = $\frac{802}{16}\times 24.8=1243.1kJ$

Thus heat released when 24.8 g of methane is burned in excess oxygen gas is 1243.1 kJ

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3 years ago

Which of the following is not balanced?

White raven [17]

Is it asking which is or isn’t balanced

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3 years ago