Asample of gas has a volume of 4.28 liters at a temperature of 10.24 degrees celcius and a pressure of 42.20 mmhg. what would be the volume at a pressure of 4.56 kpa and a temperature of 21.3 degrees celcius?

V₂  = 9.14 L

Explanation:

Given data:

Initial volume = 4.28 L

Initial pressure = 42.20 mmHg (42.20/760 = 0.056 atm)

Initial temperature = 10.24 °C (72 +273 = 283.24 K)

Final temperature = 213°C (213+273 = 486 K)

Final pressure = 4.56 KPa (4.56/101.325 = 0.045 atm)

Final volume = ?

Solution:

P₁V₁/T₁ = P₂V₂/T₂

V₂ = P₁V₁ T₂/ T₁  P₂

V₂ = 0.056 atm × 4.28 L × 486 K / 283.24 K × 0.045 atm

V₂  =  116.48 atm .L.  K  / 12.75 K . atm

V₂  = 9.14 L

the answer is a. co2, this would be colder than the : )

explanation:

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: