Question

A chemical reaction occurring in a cylinder equipped with a movable piston produces 0.621 mol of a gaseous product. If the cylinder contains 0.120 mol of gas before the reaction and has an initial volume of 2.18 mL, what is its volume after the reaction? (Assume constant pressure and temperature and that the initial amount of gas completely reacts).

a. 0.359 mL
b. 1.799 mL
c. 3.607 mL
d. 5.394 mL

Answer 1

The answer is B.
B is the most realistic answer and provides the correct one

Answer 2

The volume of the gas in the cylinder after the reaction, under constant pressure and temperature, can be calculated using the mole-to-volume ratio. The resulting volume is approximately 9.388 mL when rounded to three decimal places, which does not match any of the provided answer choices.

Step-by-step explanation:

To calculate the volume of the cylinder after the chemical reaction, which has constant pressure and temperature, we can apply the ideal gas law in a simplified form, considering the initial and final conditions. The amount of gas changes due to the reaction, and assuming complete reaction of the initial gas, we can use ratios because the temperature and pressure remain constant.

Given that the initial amount of gas is 0.120 mol with a volume of 2.18 mL and the final amount after reaction is 0.621 mol, we can set up a direct proportion between the amounts of gas and their respective volumes. The initial volume of 2.18 mL corresponds to 0.120 mol of gas. After the reaction, we have 0.621 mol of gas. To find the new volume V2:

V1 / n1 = V2 / n2
2.18 mL / 0.120 mol = V2 / 0.621 mol
V2 = (2.18 mL × 0.621 mol) / 0.120 mol
V2 = 11.2658 mL / 0.120 mol
V2 = 9.388 mL

Thus, the volume of the gas after the reaction is approximately 9.388 mL, rounded to three decimal places, which is not among the answer choices given, suggesting there might be a mistake in the question or answer choices.