Question

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2C2H2 (g) + 5O2(g) --> 4CO2(g) + 2H2O(g)
How many liters of C2H2 are required to produce 8 L of CO2 assuming the reaction is at STP?

Answer 1

According to the balanced chemical equation, 2 moles of C2H2 produce 4 moles of CO2. Therefore, 1 mole of C2H2 produces 2 moles of CO2.

At STP, 1 mole of any gas occupies 22.4 L.

So, to produce 8 L of CO2, we need (8/22.4) = 0.3571 moles of CO2.

Since 1 mole of C2H2 produces 2 moles of CO2, we need (0.3571/2) = 0.1786 moles of C2H2.

Finally, using the ideal gas law, we can calculate the volume of C2H2 required at STP:

V = nRT/P = (0.1786 mol)(0.0821 L·atm/mol·K)(273 K)/(1 atm) = 3.87 L

Therefore, 3.87 L of C2H2 are required to produce 8 L of CO2 at STP.