The molecular mass of a 2.66g sample of gas at a temperature of pressure of 845torr and occupying a volume of 0.70L is 84.16g/mol.
<h3>How to calculate molecular mass?</h3>
The molecular mass can be calculated by first calculating the number of moles using the following formula:
PV = nRT
Where;
- P = pressure
- V = volume
- n = no of moles
- R = gas law constant
- T = temperature
1.112 × 0.7 = n × 0.0821 × 300
0.7784 = 24.63n
n = 0.032mol
molecular mass = 2.66g ÷ 0.032mol
molecular mass = 84.16g/mol
Therefore, the molecular mass of a 2.66g sample of gas at a temperature of pressure of 845torr and occupying a volume of 0.70L is 84.16g/mol.
Learn more about molar mass at: brainly.com/question/14122402
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They are two representatives of the sublevels/energy levels.
Answer:
The side with lots of H+ and low pH
Explanation:
Because one of the feature of an acid is the ability to dissociate to H+.
And it has lower pH because the concentration of H+ is more than OH-
Answer:
MgO, is similar to the bonding in barium chloride, BaCl2. The bonding in each compound involves a transfer of valence electrons from the metal to the nonmetal; both metals lose all of their valence electrons
Explanation:
used goggle
We can use any solution containing chloride ions as NaCl solution or even dilute HCl due to mercurous Hg₂²⁺ is from group I cations which precipitated as chloride while Sr²⁺ is from group V
Net ionic equation:
Hg₂²⁺ + 2 Cl⁻ → Hg₂Cl₂ (white precipitate)
while SrCl₂ is soluble salt<span />
