Anonymous
Anonymous asked in Science & MathematicsChemistry · 1 month ago

the question was too long for this section so it is just down below any help is appreciated ?

A 6.05 g sample of water is introduced into a 0.838 L flask containing some C2H2 gas. The flask is heated to 215.77 °C at which temperature all of the water is converted to the gaseous phase, giving a total pressure in the flask of 19.659 atm.

 Calculate PH2O (in atm) in the flask at 215.77 °C. Report your answer to three decimal places in standard notation (i.e. 1.234 atm).

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  • 1 month ago
    Favourite answer

    Ignore the C2H2.

    P = nRT / V = ((6.05 g H2O) / (18.01532 g H2O/mol)) x (0.082057366 L atm/K mol) x

    (215.77 + 273.15) K / (0.838 L) = 16.078 atm H2O

    [There's the requested "three decimal places", although only one is justified by the rules about significant digits.]

  • david
    Lv 7
    1 month ago

    A 6.05 g sample of water is introduced into a 0.838 L flask 

      6.05 / 18.0  =  0.336 mol H2O

     

       PV = nRT

      P = nRT/V = 0.336(0.821)(1488.77)/0.838

      P = 490.079 atm

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