How does one determine a molecular formula from the empirical formula? need ! 15 a) multiply subscripts in the empirical formula by molar mass/empirical formula mass b) multiply subscripts in the empirical formula by empirical formula mass/molar mass c) multiply subscripts in the empirical formula by molar mass/grams of element d) multiply subscripts in the empirical formula by grams of element/ molar mass

A

To make the compound have the molar mass given, you need to increase the empirical formula mass to the molar mass given. An easy way to do that is to multiply by the molar mass/empirical formula mass.

aquifers are bounded above and below by impermeable rock. the driving force of groundwater movement in confined aquifers is pressure, rather than gravity.

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.