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3 years ago

Macoy Inda

Chemistry

1 answer:

Andreyy893 years ago

3 0

Answer:

? the question isn't clear

Explanation:

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Why must the number of electrons lost equal the number of electrons gained in every redox reaction

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Because energy cannot be created or destroyed, only transferred

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A container of N2O3(g) has a pressure of 0.265 atm. When the absolute temperature of the N2O3(g) is tripled, the gas completely

Rzqust [24]

Answer:

1.59 atm

Explanation:

The reaction is:

$N_{2}O_{3}(g) - - -> NO_{2}(g)+NO(g)$

The dalton's law tell us that the total pressure of a mixture of gases is the sum of the partial pressure of every gas.

So after the reaction the total pressure is:

$P_{total}=P_{NO_{2}}+P_{NO}$

we don't include $N_{2}O_{3}$ because it decomposed completely.

Assuming ideal gases

PV=nRT

P= pressure, V= volume of the container, n= mol of gas, R=constant of gases and T=temperature.

so moles of $N_{2}O_{3}$ is:

$n_{N_{2}O_{3}}=\frac{P_{1}V}{RT_{1}}$

from the reaction stoichiometry (1:1) we have that after the reaction the number of moles of each product is the same number of moles of $N_{2}O_{3}$ .

$n_{NO_{2}}=\frac{P_{1}V}{RT_{1}}$

$n_{NO}=\frac{P_{1}V}{RT_{1}}$

The partial pressure of each gas is:

$P_{NO_{2}}=\frac{n_{NO_{2}*R*T_{2}}}{V}$

$P_{NO}=\frac{n_{NO}*R*T_{2}}{V}$

so total pressure is:

$P_{total}=(n_{NO_{2}}+n_{NO})*\frac{R*T_{2}}{V}$

replacing the moles we get:

$P_{total}=(2*\frac{P_{1}V}{RT_{1}})*\frac{R*T_{2}}{V}$

We know that T2=3*T1

replacing this value in the equation we get:

$P_{total}=2*\frac{P_{1}V}{RT_{1}}*\frac{R*3T_{1}}{V}$

$P_{total}=6*P_{1} = 6*0.265 atm = 1.59 atm$

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How many (s) sublevels are present in calcium atom (Ca)?

Arlecino [84]

Answer:

nineteen atoms

Explanation:

nineteen atoms

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DETERMINE THE MASS 1.366 mol of NH3

STALIN [3.7K]

Determine the mass of each of the following amounts. a. 1.366 mol of
NH3
, b. 0.120 mol of glucose,
C6H12O6
, c. 6.94 mol barium chloride,
BaCl2
, d. 0.005 mol of propane,
C3H8

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The stopcock connecting a 1.30 L bulb containing xenon gas at a pressure of 6.15 atm, and a 4.25 L bulb containing oxygen gas at

Mrrafil [7]

Answer: False.

The final pressure in the system is 4.14 atm

Explanation: Please see the attachments below

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