:the pressure of a gas is reduced from 1200.0 mm hg to 850.0 mm hg as the volume of its container is increased by moving a piston from 85.0 ml to 350.0 ml. what would the final temperature be if the original temperature was 90.0 °c? what would the final temperature be in fahrenheit?

Initial pressure of a gas= 1200.0 mm Hg

Final pressure of a gas = 850.0 mm Hg

Initial volume of a gas = 85.0 mL

Final volume of a gas = 350.0 mL

Initial temperature of a gas = 90.0 °C = 90 + 273.15 = 363.15 K

Using the combined gas law we have,

P₁V₁/T₁ = P₂V₂/T₂

T₂ = P₂V₂T₁ / P₁V₁

where P₁, V₁, T₁ stands for initial pressure, volume and temperature respectively  and  P₂, V₂, T₂ stands for final pressure, volume and temperature respectively

Plugging the given data in the  combined gas law we get,

(1200.0 mm Hg x 85.0 mL) / 363.15 K = (850.0 mm Hg x 350.0 mL)/ T₂

T₂ = (850.0 mm Hg x 350.0 mL x 363.15 K)/ (1200.0 mm Hg x 85.0 mL)

T₂ = 1059.2 K = 1059.18 - 273.15 = 786 °C

Final temperature of a gas = 786 °C

To convert °C to  Fahrenheit

(°C × 9/5) + 32

(786°C × 9/5) + 32 = 1446.8 °F

Final temperature in Fahrenheit = 1446.8 °F

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-