In an experiment, 12.0 dm3 of oxygen, measured under room conditions, is used to burn completely 0.10 mol of propan-1-ol. what is the final volume of gas, measured under room conditions? a 7.20 dm3 b 8.40 dm3 c 16.8 dm3 d 18.00 dm3

The the correct answer is option (A).

Explanation:

12 L of oxygen gas burns 0.10 mol of propanol.(1 L = 1)

According to reaction, 2 moles of propanol gives 6 moles of then, 0.10 moles of propanol will give: moles of that is 0.30 mol.

The final volume of the gas evolved after the reaction can be determined by Ideal gas equation. Since, the reaction is taking place at room temperature the value of pressure and temperature will be:

At room temperature:

Pressure = 1 atm

Temperature , T= 293 K

The closest answer from the given options is option (A) that is 7.20

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

a electronegativity decreases beacuse the size of nucleus is bigger.