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Carbon Disulfide, CS2

Carbon Disulfide, CS2, is an important industrial substance. Its fumes can burn explosively in air to form sulfer dioxide and carbon dioxide.

CF2(g) + O2(g) (arrow) SO2(g) + CO2(g)

If 1.60 mol of CS2 burns with 5.60 mol of O2, how many mols of the excess reactant will still be present when the reaction is over.?

Also ... in the reaction of BaCO3 + 2HN03 (arrow) Ba(NO3)2 + CO2 + H2O, what mass of Ba(NO3)2 can be formed by combining 55gBaCO3 and 26gHNO3?

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Carbon Disulfide, CS2, is an important industrial substance. Its fumes can burn explosively in air to form sulfer dioxide and carbon dioxide.

You wrote:
CF2(g) + O2(g) (arrow) SO2(g) + CO2(g)

but I believe the equation should be:

CS2(g) + O2(g) --------> SO2(g) + CO2(g)

First, we balance the equation:

CS2(g) + 3 O2(g) --------> 2 SO2(g) + CO2(g)

Now, we tackle the question: If 1.60 mol of CS2 burns with 5.60 mol of O2, how many mols of the excess reactant will still be ...

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