A sample of carbon monoxide and oxygen gasses are allowed to combust in a small flask. They reaction is described by the following equation. 2CO (g) + O2 (g) + 2C02 (g) After the reaction is complete, the pressure of CO2 is 0.868 atm and the temperature is 35.0 °C in a 500.0 mL flask. How many moles of CO2 were produced assuming that the reaction went to completion? moles​

they are both synthetic elements

explanation:

d

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.