In PV = nRT, n is the number of moles. When 8 grams of oxygen are present,
n = 8/32 = 1/4
So PV = RT/4
Answer:
d
Explanation:
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Answer:
92.9 °C
Explanation:
Step 1: Given data
- Initial volume (V₁): 450. mL
- Initial temperature (T₁): 55.0 °C
- Final volume (V₂): 502 mL
Step 2: Convert 55.0 °C to Kelvin
We will use the following expression.
K = °C + 273.15 = 55.0 + 273.15 = 328.2 K
Step 3: Calculate the final temperature of the gas
If we assume constant pressure and ideal behavior, we can calculate the final temperature of the gas using Charles' law.
T₁/V₁ = T₂/V₂
T₂ = T₁ × V₂/V₁
T₂ = 328.2 K × 502 mL/450. mL = 366 K = 92.9 °C
I don't know your mc choices so I am going to go with "the number of valence electrons"
Oxidation number: the amount of electrons an atom gains, loses or shares when it forms chemical bonds. As for the valence electrons, those are the electrons that are responsible for bonds/ reactions.
The volume of water needed to prepare the solution given the data is 2.16 L
<h3>What is molarity? </h3>
This is defined as the mole of solute per unit litre of solution. Mathematically, it can be expressed as:
Molarity = mole / Volume
<h3>How to determine the mole of CaCO₃</h3>
- Mass of CaCO₃ = 756 g
- Molar mass of CaCO₃ = 100.1 g/mol
- Mole of CaCO₃ =?
Mole = mass / molar mass
Mole of CaCO₃ = 756 / 100.1
Mole of CaCO₃ = 7.55 moles
<h3>How to determine the volume </h3>
- Mole of CaCO₃ = 7.55 moles
- Molarity = 3.5 M
- Volume = ?
Volume = mole / molarity
Volume = 7.55 / 3.5
Volume = 2.16 L
Learn more about molarity:
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