Question

PLEASE ASNWER QUICK!!!! AND RIGHT ANSWERS!! 50 POINTS!!

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?
L C2H2

Answer 1

3.95 L

Step-by-step explanation:

To solve this problem, we need to use stoichiometry and the ideal gas law to determine the amount of C2H2 required to produce 8 L of CO2 at STP.

First, we need to determine the number of moles of CO2 produced from 8 L at STP. The molar volume of an ideal gas at STP is 22.4 L/mol, so:

8 L CO2 * (1 mol CO2 / 22.4 L CO2) = 0.357 mol CO2

Next, we can use the balanced chemical equation to determine the number of moles of C2H2 required to produce 0.357 mol CO2. From the balanced equation, we see that 2 moles of C2H2 produce 4 moles of CO2, so:

2 mol C2H2 / 4 mol CO2 = 0.5 mol C2H2 / mol CO2

0.357 mol CO2 * (0.5 mol C2H2 / mol CO2) = 0.179 mol C2H2

Finally, we can use the ideal gas law to convert the number of moles of C2H2 to volume at STP. The ideal gas law is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. At STP, the pressure is 1 atm and the temperature is 273 K, so:

V = nRT / P = (0.179 mol) * (0.0821 Latm/(molK)) * (273 K) / (1 atm) = 3.95 L

Therefore, 3.95 L of C2H2 are required to produce 8 L of CO2 at STP.