Calculate the pressure in atmospheres exerted by 10.0moles of hydrogen gas at 293 kelvins if it is stored in a 7.50 liter container. your value should be a decimal number written to three significant figures. given: r= 0.08205 liter x atmosphere/mole x kelvin

To determine the pressure of the gas, we need an equation which would relate pressure to the values given like the number of moles, temperature and the volume of the system. For simplicity, we can assume that the hydrogen gas is an ideal gas so we use the equation PV=nRT where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant and T is the temperature. 

PV = nRT
P = nRT / V
P = 10.0 mol  (0.08205 L - atm / mol-K) (293 K) / 7.50 L
P = 32.0542 atm
 Therefore, the pressure of the system would be 32.054 atm

Dot structures do not show the distribution of electrons in orbitals and take up a lot of space.

Arrow and line diagrams take up a lot of space and make it difficult to count electrons.

Written configurations make it easy to lose count of electrons and do not show the distribution of electrons in orbitals.

(re-write in your own words this is off engenuity)