Oxygen has a density of 1.43 g/l at stp. what is the density of oxygen at 1.30 atm?

Explanation:

It is given that pressure is 1.30 atm.

So, at STP temperature will be 273.15 K. And, according to the ideal gas equation:

                         PV = nRT ........ (1)

And,    Density =

or,               Volume = ....... (2)

Putting equation (2) is equation (1) we get the following.

                                 PV = nRT

Molar mass of oxygen is 32 g/mol. Now, putting the given values into the above equation to calculate density as follows.

                    Density =   g/L

                                  = 1.855 g/L

Thus, we can conclude that density of oxygen at 1.30 atm is 1.855 g/L.

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.