Answer:
15.9gmol⁻¹
The gas could have been methane when we compare the two molecular masses.
Oxygen gas, O₂ also shares this same number for its molecular mass. This would be the reason why it would not be methane.
Explanation:
Given parameters:
Volume of gas at STP = 2.0L or 2.0dm³(1L = dm³)
Mass of the gas = 1.43g
Unknown:
Molecular mass of the gas = ?
Solution
We can find the number of moles using the mole concept according to the equation below:
number of moles = ³⁻¹
number of moles =
number of moles = 0.089mol
Using this obtained number of moles, we can derive the molecular mass of the compound by using the relationship between mass and number of moles according to the equation below:
molecular mass =
molecular mass =
molecular mass of the gas = 15.9gmol⁻¹
The formula of methane gas is CH₄.
Let's calculate the molecular mass of methane using these atomic masses:
C = 12g and H = 1g
The molecular mass = 12 + (1x4) = 16gmol⁻¹
The gas could have been methane when we compare the two molecular masses.
Oxygen gas, O₂ also shares this same number for its molecular mass. This would be the reason why it would not be methane.
Answer:
It has a greater concentration of hydroxide ion than hydronium ions.
<u>Answer:</u>
<em>A - It will increase</em>
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<u>Explanation:</u>
Take for instance,
The number of particles (10000) present initially is less in a per unit volume say in 1 mL.
The number of particles increases (20000) in the same volume 1mL
.
So, the pressure will increase in the container since 10000 particles is present in a low volume of 0.5 mL now.
We know as volume decreases the pressure will increase as per Boyle’s law.
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Answer:
neutron
Explanation:
neutron and proton has approximately the same mass .proton is positively charged but neutron has no charge