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anonymous

  • one year ago

How many liters of carbon dioxide can be produced if 37.8 grams of carbon disulfide react with excess oxygen gas at 28.85 degrees Celsius and 1.02 atmospheres? CS2(l) + 3O2(g) yields CO2(g) + 2SO2(g) 2.78 liters 5.95 liters 12.1 liters 11.9 liters

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  1. anonymous
    • one year ago
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    @nincompoop @THESTRUGGLER @TheSmartOne

  2. anonymous
    • one year ago
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    @Mertsj

  3. taramgrant0543664
    • one year ago
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    Your first step is to take the amount of carbon disulfide and divide be the molar mass so 37.8/ 76.14= number of moles of carbon disulfide

  4. taramgrant0543664
    • one year ago
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    Once you find the moles of carbon disulfide you relate it to the carbon dioxide the stoichimometric coefficients are both 1:1 so the moles of carbon disulfide are the same as the carbon dioxide

  5. taramgrant0543664
    • one year ago
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    Since you have the moles of carbon dioxide you can use the ideal gas formula PV=nRT But first you have to switch Celsius to Kalvin. To do this you take 28.85 and add 273.15 to get your temperature as 302K

  6. taramgrant0543664
    • one year ago
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    P is pressure so that's 1.02 atm V is the volume you are trying to find n is the moles of carbon dioxide R is the ideal gas constant 0.082 T is the temperature in Kalvin so that's the 302K

  7. taramgrant0543664
    • one year ago
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    Are you understanding what I put? @jammy987

  8. anonymous
    • one year ago
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    ok so that answer would be c? @taramgrant0543664

  9. taramgrant0543664
    • one year ago
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    Yes it would be c

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