Calculate to three significant digits the density of dinitrogen difluoride gas at exactly 30 °c and exactly 1 atm. you can assume dinitrogen difluoride gas behaves as an ideal gas under these conditions

2.66 g/L

Explanation:

Data

As we have the compound we calculate the molar mass

they tell us that behaves like an ideal gas, therefore we can apply the equation of ideal gases

To apply this equation we lack several data, and within the variables of the equation there is no density that is what we need to find

But we can modify it in the following way so that it is based on the data we have

density formula

from this formula we cleared the mass

The formula for calculating moles is

In this formula the mass also appears so we can substitute the variable mass for

Replace in the equation of ideal gases, the variable mol (n) by

Now that we have the equation based on the data we have, we clear the density

As the volume appears on both sides of the equation we can simplify this term

the density of dinitrogen difluoride gas at exactly 30 °C and exactly 1 atm is 2.66g/L

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