ICK
exercise 13.2 A sample of neon to be used in neon sign has a volume of 1.51 L at a pressure of 635 torr.
Calculate the volume of the gas after it is pumped into the glass tubes of the sign, where it shows a pressure of 785 torr.

The new volume, after increasing the pressure to 785 torr, will be 1.22 L

Explanation:

Step 1: Data given

Volume of neon sign is 1.51 L

Pressure of the neon gas = 635 torr

The pressure increases to 785 torr

Step 2: Calculate the volume

P1*V1 = P2*V2

⇒with P1 = the initial pressure of the gas = 635 torr

⇒with V1 = the initial volume of the gas = 1.51 L

⇒with P2 = the increased pressure = 785 torr

⇒with V2 = the new volume = TO BE DETERMINED

635 torr * 1.51 L = 785 torr * V2

V2 = (635 torr * 1.51 L ) / 785 torr

V2 = 1.22 L

The new volume, after increasing the pressure to 785 torr, will be 1.22 L

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

its first and third is your answer i did the qustion the fourth isnt right