An unknown compound contains only carbon, hydrogen, and oxygen (cxhyoz). combustion of 4.50 g of this compound produced 6.60 g of carbon dioxide and 2.70 g of water. how many moles of hydrogen, h, were in the original sample

The number of moles of Hydrogen H  that were in the original sample is

0.30 moles

               CxHyOz  + O2 →  CO2 + H2O

   moles= mass/molar mass

        =  6.60g/44 g/mol=0.15 moles

  molar mass= mass/  moles

 =  4.50/0.15=  30 g/mol

 C =x(12 g/mol)  if  x=1  then c= 12  g/mol

  H= y (1 g/mol) if Y=1 then H=1 g/mol

   O=Z(16g/mol) if O=16 then O= 16g/mol

 the formula of the compound from the value of X,y and  z above = CHO

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.