Answer:
See answer below
Explanation:
Hi there,
This question is employing the Gas Laws, specifically the relationship between internal gaseous pressure and temperature, when volume and gas quantity are constant; Gay-Lussac's Law:
[tex]\frac{P}{T} =k[/tex] or [tex]\frac{P_1}{T_1} =\frac{P_2}{T_2}[/tex]
However, we will need to convert the pressures and temperatures into standard units. Pressure must be put in terms of (atm) and temperature in Kelvin (K).
[tex]P_1=55kPa*\frac{1 \ atm}{101.3 \ kPa} = 0.543 \ atm\\T_1 = -100 \ C + 273.15 = 173.15 \ K\\T_2 = 200 \ C + 273.15 = 473.15 \ K[/tex]
Now, solve for [tex]P_2[/tex] as this is what was asked for:
[tex]P_2 = T_2\frac{P_1}{T_1}= (473.15K)*\frac{0.543 \ atm}{173.15K} = 1.484 \ atm[/tex]
If needed, convert back into kPa, so 1.484 * 101.3 kPa = 150.3 kPa.
thanks,
