What mass of sulfur has to burn to produce 4.5l so2 at 300°c and 101 kpa in the following reaction?

a. 13.5 g s
b. 3.07 g s
c. 68.8 g s
d. 41.0 g s

The correct answer is option B.

Explanation:

Pressure of the gas = P = 101 kPa = 0.9968 atm

Volume of the gas = V = 4.5 L

Temperature of the gas = T = 300°C = 573.15 K

Moles of sulfur dioxide = n

n = 0.09533 mol

According to reaction , 1 mol sulfur dioxide is obtained from 1 mol of sulfur.

Then 0.09533 mol will be obtained from:

Mass of 0.09533 moles of sulfur = 0.09533 mol × 32 g/mol= 3.07 g

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e

the answer is na (sodium)