4. A constant volume of gas has a pressure of ​98.3 kPa​ at ​497 K​ . Determine the temperature of the gas if the pressure is increased to ​182.5 kPa​ . a) Should the temperature of the gas increase or decrease? b) Using Kinetic Molecular Theory (KMT), explain your answer to (a). ​HINT​: What happens to the particles? c) Determine the final temperature of the gas. P​ 1​= P​ 2​= T​ 1​= T​ 2​= k = k =

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year

idk i'm not smart

explanation:

t h

stratosphere, is the answer for (apex)

option c: 1605.1 kj

the balanced chemical reaction for combustion of methane is as follows:

here, enthalpy formation of is -74.7 kj/mol, 0 kj/mol, -393.5 kj/mol and -241.82 kj/mol respectively.

the heat released or can be calculated as follow:

putting the values,

thus, heat released by combustion of 1 mol of methane is 802.54 kj/mol. thus, for 2 mol, heat released will be:

therefore, heat released by the combustion of 2 mol of methane is 1605.1 kj.