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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 11.9 liters 12.2 liters

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  1. anonymous
    • one year ago
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    @sweetburger

  2. Photon336
    • one year ago
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    @jammy987 you know right away from the question what your limiting reagent is can you tell what that is?

  3. anonymous
    • one year ago
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    @photon336 so the answer would be b

  4. Photon336
    • one year ago
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    Carbon di sulfide is our limiting reagent so you need use that to calculate the moles of carbon dioxide produced. do you know how to do this?

  5. Photon336
    • one year ago
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    \[\frac{ 1 mol CS _{2} }{76 g } * 37.8 g CS _{2} = moles CS _{2}\]

  6. Photon336
    • one year ago
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    you first need to ensure that your chemical equation is balanced first then calculate the number of moles of CS2 once you get the moles of CS2 you must multiply by the molar ratio to get how much CO2 was produced. \[Mol CS _{2} * \frac{ CO _{2}}{ CS _{2} } = Mol CO _{2}\] then tell me what you get from this.

  7. Photon336
    • one year ago
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    Then when you get the moles of CO2 use the formula below. \[PV = nRT \] You're solving for volume. You know pressure, Temperature, and R= 0.082 and n. But make sure your temperature is in Kelvin not Celsius to do that its K = C+273 \[\frac{ nRT }{ P }= Volume \in liters \] for carbon dioxide

  8. anonymous
    • one year ago
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    yes so it would be c?@photon336

  9. anonymous
    • one year ago
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    @photon336

  10. JoannaBlackwelder
    • one year ago
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    I didn't get c, although I got close to that. How did you get c?

  11. anonymous
    • one year ago
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    @JoannaBlackwelder oh it was d

  12. JoannaBlackwelder
    • one year ago
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    Yeah, that's what I got. :-)

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