A gas is at a pressure of 12 atm, a volume of 23 L, and a temperature of 200 K. If the pressure is raised to 14 atm, and the temperature is increased to 300 K. What is the new volume of the gas? (Show your work, including formula used)

≅ 30 Liters (1 sig. fig. based on Temp values 200K & 200K)

Explanation:

P₁ = 12 atm      =>    P₂ = 14 atm   Increase P  =>  Decrease V  => (12atm/14atm)

V₁ = 23 Liters  =>    V₂ =   ?          

T₁ = 200 K       =>    T₂ = 300 K    Increase T  =>  Increase V  =>  (300K/200K)

V₂ = V₁(P₁/P₂)(T₂/T₁) = 23L(12atm/14atm)(300K/200K) = 29.57143 L (Calc. Ans.)

≅ 30 Liters (1 sig. fig. based on Temp values 200K & 200K)

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: