If a gas in a closed container is pressurized from 14.9 atm to 16.5 atm and its original temperature was 33.1 °C, what would the final temperature of the gas be?

339K

Explanation:

Initial pressure P1 = 14.9 atm

Final pressure P2 = 16.5 atm

Original temperature T1 = 33.1 °C

Convert Celsius to Kelvin

(33.1°C + 273 = 306.1K)

Final temperature T2 = ?

Apply the formula for Pressure's law

P1/T1.= P2/T2

14.9atm/306.1K = 16.5atm/ T2

To get T2, cross multiply

14.9 x T2 = 16.5 x 306.1

14.9T2 = 5050.65

T2 = (5050.65/14.9)

T2 = 339K

Thus, the final temperature of the gas would be 339K

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

lol idk man i guess u gotta ask bill nye the science guy