Hydrogen gas at a temperature of 22.0°C that is confined in a 5.00L cylinder exerts a pressure of 4.20atm. If the gas is released into a 10.0L reaction vessel at a temperature of 33.6°C, what will be the pressure inside the reaction vessel?

The pressure inside the reaction vessel is 2.18 atm

Explanation:

Step 1: Data given

The temperature = 22.0 °C = 295.15 K

Pressure = 4.20 atm

Volume = 5.0 L

Volume increased to 10.0 L

Temperature increased to 33.6 °C = 306.75K

Step 2: Calculate the new pressure

P1 * V1 / T1 = P2*V2 / T2

⇒with P1 = the initial pressure = 4.20 atm

⇒with V1 = the initial volume = 5.0 L

⇒with T1 = the initial temperature = 295.15 K

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 10.0L

⇒with T2 = the increased temperature = 306.75 K

(4.20 atm * 5.0 L) / 295.15 K = ( P2 * 10.0 L ) / 306.75 K

P2 = (4.20 * 5.0 L * 306.75 K) / (295.15 K * 10.0 L)

P2 = 2.18 atm

The pressure inside the reaction vessel is 2.18 atm

a. a primary source combines several different accounts of an event. b. a primary source generally benefits from having been written after an event.

explanation:

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3