A sample of nitrogen gas occupies a volume of 2.55 L when it is at 755 mm Hg and 23 degrees Celsius. Use this information to determine the moles of nitrogen gas present. Volume is increased to 4.10 L and temperature is decreased to 18 degrees Celsius. Calculate the final pressure

The final pressure is 461.6 mm Hg

Explanation:

Step 1:Data given

Volume of N2 = 2.55L

Pressure N2 = 755 mm Hg

Temperature = 23.0 °C

New volume = 4.10 L

Temperature = 18.0 °C

Step 2: Calculate the fina pressure

P1V1/T1 = P2V2/T2

P2 = P1V1/T1 * T2/V2

⇒ with P1 = initial pressure = 755/760 atm =0.993421 atm

⇒ with V1 = the initial volume = 2.55L

⇒ with T1 = the initial temperature = 23.0 °C = 296 K

⇒ with P2 = The final pressure

⇒with V2 = the new volume = 4.10 L

⇒with T2 = the new temperature = 18.0 °C = 291 K

P2 = 755 mm *2.55 L *296K/(291 K* 4.10 L) = 461.6 mm Hg

The final pressure is 461.6 mm Hg

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

indium, and thallium have three electrons i think