find the volume, in liters, of 980 mg of CS2(s) at STP?

please help!

i need EXPLANATIONS of how to do this stuff! <3

3 Answers

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  • Dr W
    Lv 7
    1 decade ago
    Best Answer

    are you sure about this question?

    CS2 is carbon disulfide. it has a melting point of -112C and a boiling point of +46C at P = 1 atm. T in STP is 0 C... so CS2 is a liquid at STP.. you wrote CS2(s)...and the other answerer used the ideal gas law.. CS2(g)...

    *************

    from here...

    http://www.sigmaaldrich.com/catalog/ProductDetail....

    CS2(l) has a density of 1.266 g/mL at 25C.. not sure what it is at 0 C (STP).. but it's probably close to 1.266 g/mL...

    980 mg x (1 g / 1000 mg) x (1 mL / 1.266g) = 1.241 mL...again at 25C

  • 1 decade ago

    Atomic weights: C=12 S=32 CS2=76

    980 mg = 0.980g

    0.980gCS2 x 1molCS2/76gCS2 x 22,400mLCS2/1molCS2 = 289 mL CS2 to three significant figures

    22,400 mL = 22.4 L is the molar volume of any perfect gas at STP.

  • 1 decade ago

    Use the ideal gas equation: PV = nRT

    P is the pressure in atmospheres

    V is the volume in liters

    n is the number of moles of gas

    R is the gas constant: 0.08205 liter-atm/mole degree Kelvin

    T is the temperature in Kelvin

    STP is 0 degrees Celsius, 1 atmosphere.

    Convert to Kelvin: degrees K = 0 C +273 = 273 K

    V = nRT/P = (n X0.08205 X 273)/ 1atm

    The number of moles, n, will be the grams of CS2 divided by the mole weight of CS2 - that is

    0.980 grams/(12+32+32) = 0.98g/76 g/mole = 0.01289 moles of CS2

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