A mixture of two gases, 0.01 mol of C4H10(g) and 0.065 mol of O2(g), is pumped into a cylinder with — States of Matter Chemistry Question
Question
A mixture of two gases, 0.01 mol of C4H10(g) and 0.065 mol of O2(g), is pumped into a cylinder with a movable piston, as shown above. [VISUAL] The mixture, originally at 20°C and 1.0 atm, is sparked and the reaction represented below occurs.
2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g)
Which of the following is true after the product gases return to the original temperature and pressure, and why will the change occur? (Assume all gases behave ideally.)
The piston will be higher than its original position because there are more moles of gas in the cylinder after the reaction.
The piston will be lower than its original position because there are fewer moles of gas in the cylinder after the reaction.
The piston will be at the same position because the temperature and pressure are returned to their original values.
The piston will be at the same position because the gas behaves ideally.