Agas at 250 k has a pressure of 0.00008 pa. if the pressure drops to 0.00002 pa, what is the new temperature? 500 k 1000 k 125 k 62.5 k

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If a gas at 250 K has a pressure of 0.00008 Pa and the pressure drops to 0.00002 Pa, 62.5 K is the new temperature

Explanation: -

Initial Pressure P₁ = 0.00008 Pa

Final Pressure P₂ = 0.00002 Pa

Initial Temperature T₁ = 250 K

Since the volume is not mentioned, it remains constant.

So initial Volume V₁ = Final volume V₂

Now using the combined gas equation

=

Final Temperature T₂ =

Plugging in the values,

T₂ =

As V₂ = V₁, they cancel each other.

T₂ = 62.5 K

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: