Hello!
At
Standard Pressure and Temperature, an ideal gas has a molar density of
0,04464 mol/L.So, we need to apply a simple conversion factor to calculate the density of Sulfur Dioxide using the molar mass of Sulfur Dioxide.

So, the Density of Sulfur Dioxide (SO₂) at STP is
2,8599 g/LHave a nice day!
Answer:
A
Explanation:
molarity=moles of solute/liter of solution
molarity=0.26/0.3
molarity=0.87molar
Explanation:
Atoms of metals do not hold their electrons to themselves. Instead they allow them to float around them delocalised. This is important because it is this characteristic that allows metals to be good conductors of electricity since electrons are free to move around to carry a charge.
please mark it brainliest
Answer:
When a gas occupies a smaller volume, it exerts a higher pressure; when it occupies a larger volume, it exerts a lower pressure (assuming the amount of gas and the temperature do not change). Since P and V are inversely proportional, a graph of 1/P vs. V is linear.
Explanation:
<h2><u><em>
This is all I know.</em></u></h2><h2><u><em>
Hope it helps~</em></u></h2><h2><u><em>
Good luck with your work!!~</em></u></h2>