Ga sealed container holds 0.020 moles of nitrogen (n2) gas, at a pressure of 1.5 atmospheres and a temperature of 290 k. the atomic mass of nitrogen is 14.0 g/mol. the boltzmann constant is 1.38 × 10-23 j/k and the ideal gas constant is r = 8.314 j/ mol · k = 0.0821 l · atm/mol · k. the mass density of the gas is closest to

Explanation:

The given data is as follows.

        n = 0.020 moles,    P = 1.5 atm

        T = 290 K,      molar mass of nitrogen = 14.0 g/mol

         R = 8.314 J/mol,         d = ?

It is known that  the relation between density, pressure, and temperature is as follows.

                 P =

Putting the given values into the above relation and calculate the density as follows.

              P =

             1.5 atm =

                    d =

                      = g

Thus, we can conclude that density of the given gas is g.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons