Using the balanced equation, 2 C2H2(g)+5 O2(g) yields 4 CO2(g)+2 H2O(g), at STP if 1mol of C2H2 burned in unlimited oxygen and the theoretical yield of carbon dioxide in liters at STP is 44.8 liters of carbon dioxide, and if 28.5 liters of carbon dioxide is produce to give you 63.62% yield, what is the actual yield?

Question

Using the balanced equation, 2 C2H2(g)+5 O2(g) yields 4 CO2(g)+2 H2O(g), at STP if 1mol of C2H2 burned in unlimited oxygen and the theoretical yield of carbon dioxide in liters at STP is 44.8 liters of carbon dioxide, and if 28.5 liters of carbon dioxide is produce to give you 63.62% yield, what is the actual yield?

Answer 1

The actual yield is 28.5 L according to the problem.

Try it. Isn't
(28.5/44.8)*100 = 63.62%? Sure is.

Answer 2

To find the actual yield of the reaction, we need to calculate the percentage yield first. Percentage yield is calculated by dividing the actual yield by the theoretical yield and multiplying by 100.

Given:
The theoretical yield of carbon dioxide (CO2) is 44.8 liters.
The percentage yield is 63.62%.

Let's calculate the actual yield using the given information:

Step 1: Convert the percentage yield to a decimal:
Percentage yield = 63.62 / 100 = 0.6362

Step 2: Calculate the actual yield:
Actual yield = Percentage yield * Theoretical yield
Actual yield = 0.6362 * 44.8 liters
Actual yield = 28.52656 liters

Therefore, the actual yield of carbon dioxide is approximately 28.53 liters at STP.