Hydrogen peroxide decomposes to give water and oxygen gas according to the equation below. If 3.0 moles of hydrogen peroxide decompose, what volume of oxygen gas is produced at a pressure of 1.0 atm and a temperature of 23 °C? 2 H2O2(l) → 2 H2O(l) + O2(g)

Answers

Answer 1

Answer:

When 3.0 moles of hydrogen peroxide decompose at 1.0 atm and 23°C, approximately 36.78 liters of oxygen gas are produced according to the ideal gas law.

What volume of oxygen gas is produced at a pressure of 1.0 atm and a temperature of 23 °C?

To find the volume of oxygen gas produced when 3.0 moles of hydrogen peroxide decompose at a pressure of 1.0 atm and a temperature of 23°C, you can use the ideal gas law:

PV = nRT

Where:

- P is the pressure (1.0 atm).

- V is the volume (what we want to find).

- n is the number of moles of gas (1.5 moles of O2 since 1 mole of O2 is produced for every 2 moles of H2O2).

- R is the ideal gas constant (approximately 0.0821 L.atm/mol.K).

- T is the temperature in Kelvin (23°C needs to be converted to Kelvin, which is 296.15 K).

First, calculate the number of moles of O2 produced:

n = 3.0 moles of H2O2 * (1 mole of O2 / 2 moles of H2O2) = 1.5 moles of O2

Now, plug in the values into the ideal gas law and solve for V:

1.0 atm * V = 1.5 moles * 0.0821 L·atm/mol·K * 296.15 K

Now, calculate the volume:

V = (1.5 moles * 0.0821 L·atm/mol·K * 296.15 K) / 1.0 atm

Calculate the volume:

V ≈ 36.78 L

So, the volume of oxygen gas produced when 3.0 moles of hydrogen peroxide decompose at 1.0 atm and 23°C is approximately 36.78 liters.

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Answer 2

Answer: First you need to use stoichiometry to find how many moles of oxygen is produced from the reaction. To do this you need to multiply the number of moles of hydrogen peroxide by the molar ratio which is 1/2 since 1 mole of O₂ is produced from 1 mole of H₂O₂. 3mol H₂O₂x(1mol O₂/2mol H₂O₂)=1.5mol O₂
you you need to you the ideal gas law (PV=nRT) to find the volume of gas produced. V=nRT/P
n=1.5mol
R=0.08206atmL/molK
T=23°C (turn that into 296K)
P=1atm
V=(1.5molx0.08206atmL/molK)/1atm
V=0.1231L

I hope this helps.

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Answers

The answer is 1/8.

Half-life is the time required for the amount of a sample to half its value.
To calculate this, we will use the following formulas:
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♡♡Hope I helped!!! :)♡♡

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Answers

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Calcium reacts with cold water to form calcium hydroxide and hydrogen gas:

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Answers

Answer:

Explanation:

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gold ...is only gold

2. air IS a mixture of various gases.....nitrogen , oxygen, co2 etc

Final answer:

Option 2: The air in your room. The air in your room is an example of a mixture because it consists of various gases that can be separated from each other.

Explanation:

The correct answer is Option 2: The air in your room.

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Answers

Answer : (2) Ethanoic acid has the lowest vapor pressure at $75^(0)C$ .

Explanation :

Vapor pressure is the pressure which is exerted by vapor when the vapor form is in equilibrium with the solid or liquid form.

Boiling point is the temperature in which the vapor pressure of liquid is equal to the atmospheric pressure.

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The image of graph of vapor pressure vs temperature is attached below.

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Propanone: is a ketone and has an electronegative oxygen attached to a carbon, but does not exhibit hydrogen bonding since the O is not attached to a hydrogen.
Ethanol: Like water exhibits hydrogen bonding, not as strong but more dispersion forces.

Next we must understand boiling points
Water: 100˚C
Ethanoic Acid: 118˚C
Propanone: 56˚C
Ethanol: 78˚C
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