Start with the ideal gas equation, <span><span><span>PV=nRT</span> </span><span>PV=nRT</span></span>
and rearrange for pressure to get <span><span><span>p=<span><span>nRT</span>V </span></span> </span><span>p=<span><span>nRT</span>V</span></span></span>
. You have all the necessary variables in their proper units, so plug em' into the equation to solve for pressure in units of atmospheres.
All that needs to be done now is converting atmospheres to mm <span><span><span>Hg</span> </span><span>Hg</span></span>
.
<span><span><span>1.23 atm∗<span><span>760 mm Hg</span><span>1 atm</span> </span>=935 mm Hg</span> </span><span>1.23 atm∗<span><span>760 mm Hg</span><span>1 atm</span></span>=935 mm Hg</span></span>
.
That value makes sense, since the original pressure in atmospheres was above 1, the pressure in mm <span><span><span>Hg</span> </span><span>Hg</span></span>
will be above 760.
The same number of atoms of each element must appear on both sides of a chemical equation. However, simply writing down the chemical formulas of reactants and products does not always result in equal numbers of atoms. You have to balance the equation to make the number of atoms equal on each side of an equation.
