hi, i am having problem with the following problems: a gaseous binary compound h

Question

hi, i am having problem with the following problems: a gaseous binary compound has a vapor density that is 1.94times that of oxygen at the same temperature and pressure. When1.39 g of the gas is burned in an excess of oxygen, 1.21 g of wateris formed, removing all the hydrogen originally present
a.estimate the molecular mass of the gaseous compound b.how many H atomes are there in a molecule of thecoumpound c.wat is the maximum possible value of the atomic mass of thesecond element in the compound? d.are other values possible for the atomic mass of the secondelement? Usa a table of atomic masses to identify the element thatbest fits the date e.what is the molecular formula of the compound?
thanks! a gaseous binary compound has a vapor density that is 1.94times that of oxygen at the same temperature and pressure. When1.39 g of the gas is burned in an excess of oxygen, 1.21 g of wateris formed, removing all the hydrogen originally present
a.estimate the molecular mass of the gaseous compound b.how many H atomes are there in a molecule of thecoumpound c.wat is the maximum possible value of the atomic mass of thesecond element in the compound? d.are other values possible for the atomic mass of the secondelement? Usa a table of atomic masses to identify the element thatbest fits the date e.what is the molecular formula of the compound?
thanks!

Explanation / Answer

We Know that :    According to the given data :      Binary compound contains one of theelement is Hydrogen let the other element is A       AxHy ----Binary compound      AH + O2 ------> AO + H2O    ( AO is the oxide of the element )      Molecular weight = 1.94 xO2                              = 1.94 x 32 g /mol          (Molecular weight of O2 = 32 g / mol )                              = 62.08 g / mol                              = 62.1 g / mol               The weight of water obtained from the reaction= 1.21 g      number of moles of water formed inthe reaction = 1.21 g / 18 g / mol                                                                                = 0.06722 mol The actual number of moles of Hydrogen present in the binarycompound is                                                                                            = 2x( number of moles of waterformed)           number of moles of hydrogen inthe binary compound = 0.1344 moles            weight of the binary compound is 1.39 g       number of moles of binary compound = 1.39 g / 62.1 g / mol                                                                      = 0.022 mol          weight of thehydrogen in the compound   0.1344 mole x 1 g / mol                                                                       = 0.1344 g           weightof the other element in the binary compound = 1.39 g - 0.1344g                                                                                         = 1.2556 g           number of moles of the other element constitutes = 0.022 mol                Molecular mass of the other element = 56 g /mol                 xA + y ( 1 ) = 62.1               let us assume the values of x and y to be 2 , 6 bysubstituting the values it satisfy the condition as the solution ofthe answer.                    Form the inspection of the molecular weight of the otherelement = 56 g / mol              The element is most probable is Si                      The molecular formula of the compound is Si2H6                                        

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

---