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)
Stacey Warren - Expert brainly.com
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@nincompoop @THESTRUGGLER @TheSmartOne
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
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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
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
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