Warming a gas at constant volume and a pressure of 1.50 atm from 27 degrees Celsius to 127 degrees Celsius gives a final pressure of

Final pressure of gas = 2 atm

Explanation:

Given data:

Initial pressure of gas = 1.50 atm

Initial temperature = 27°C

Final temperature = 127°C

Final pressure of gas = ?

Solution:

Initial temperature = 27°C (27+273 = 300 K)

Final temperature = 127°C ( 127+273 = 400 K)

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

1.50  atm / 300 K = P₂/400 K

P₂ = 1.50 atm × 400 K / 300 K

P₂ = 600 atm. K /300 K

P₂ = 2 atm

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:

i would say b

explanation:

but i think i would need more information than that