1. A pycnometer, nominally 10 ml, was found to have a volume of 9.9872 ml, when filled
exactly to the top of the capillary in the stopper. The pycnometer was filled with
deionized (pure) water, and weighed. The mass of the filled pycnometer was found to be
23.1148 g. The pycnometer empty was weighed, and found to have a mass of 13.1455 g.
Calculate the density of the water. What temperature, in °C, was the experiment
performed at?

Answer : (1) :-

Volume of water filled in the pycnometer is given as = 9.9872 mL.

Mass of pycnometer when filled with water = 23.1148 g.

Mass of empty pycnometer = 13.1455 g.

So, mass of water = (23.1148 - 13.1455) g. = 9.9693 g.

We know that,

   Density = Mass / Volume = (9.9693 g.) / (9.9872 mL) = 0.998 g/mL.

It is observed that the density of water is evaluated to be 0.998 g/mL. We know that, at 4℃ the density of water becomes maximum i.e. 1 g/mL. On the other hand the temperature at which the density of water is 0.998 g/mL is 0℃. Therefore, it can be concluded that the experiment was performed at a temperature of 0℃.

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24