What volume (L) would be produced from 1.5x1025 molecules of CO2 at STP?

557.7 L

Explanation:

1 mol → 6.02×10²³ molecules at STP produces 22.4L

Therefore, we need to know how many moles are 1.5 ×10²⁵ molecules

( 1.5 ×10²⁵ molecules / 6.02×10²³ molecules) . 1 mol = 24.9 moles

Let's make a rule of three:

1 mol can produce at STP a volume of 22.4 L

24.9 moles may produce at STP a volume of (24.9 . 22.4)/1 = 557.7 L

Let's verify by the Ideal Gases Law

P . V = n . R . T → V = (n . R . T ) / P

STP → Pressure = 1 atm, T = 273 K

V = (24.9 mol . 0.082 L.atm/mol.K . 273 K) / 1 atm → 557.4 L

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:

b

explanation:

mitosis