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9 March, 06:38

If 0.84 mol of CS2 reacts with oxygen completely according to the equation CS2 (ℓ) + 3 O2 (g) → CO2 (g) + 2 SO2 (g) what volume (total) would the products occupy if they were measured at STP?

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  1. 9 March, 10:28
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    The products will occupy a volume of 56.448 L when measured at STP

    Explanation:

    The first thing to check here is the mole ratio of the reactant in question to the product.

    From the chemical equation, we can see that 1 mole of CS2 gave a total mole of 3 moles of the products (1 mole of carbon iv oxide and 2 moles of sulphur iv oxide)

    Now if 1 mole of reactant can give 3 moles of the products,

    then 0.84 mole of reactant will give 3 * 0.84 moles of the product = 2.52 moles of the products

    We are told to calculate the total volume.

    At STP, 1 mole of a gaseous substance will occupy a volume of 22.4L or 22.4 dm^3 (liters and dm^3 are same)

    This means that 2.52 moles will occupy a volume of 22.4 * 2.52 = 56.448L
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