The volume of a gas is 550 ml at 960 mm hg and 200.0°C. What volume would the pressure of the gas be 830 mm Hg if the temperature is reduced to 150°C?

V₂ = 568.9 mL

Explanation:

Given data:

Volume of gas = 550 mL

Pressure of a gas = 960 mmHg

Temperature = 200.0°C ( 200+273 = 473 K)

Final volume = ?

Final pressure = 830 mmHg

Final temperature = 150°C (150+273 = 423 K)

Solution:

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 960 mmHg × 550 mL × 423 K / 473 K ×830 mmHg

V₂ = 223344000 mL / 392590

V₂ = 568.9 mL

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

answer; the numbers of valence electrons in the acetic acid molecule (ch3co2h) is 24;