What is the pressure of a gas that began at 38 torr, and 500l and is changed to occupy a volume of 677 l?

P₂ = 28.5 torr

Explanation:

Given data:

Initial pressure = 38 torr

Initial volume = 500 L

Final volume = 677 L

Final pressure = ?

Solution:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = Initial volume

P₂ = Final pressure

V₂ = Final volume

Now we will put the vales in formula.

P₁V₁ = P₂V₂

P₂ = P₁V₁ /V₂

P₂ = 38 torr × 500 L / 667 L

P₂ = 19000 torr. L / 667 L

P₂ = 28.5 torr

- calcium has greater affinity to bond with electron receptors than hydrogen does and hence, it has the ability to replace hydrogen in most of its compounds.

- lithium has 2 valence electrons in the product because it can make only 1 bond with hydrogen. beryllium has 4 valence electrons in the product because it can only make 2 bonds. it has fewer electrons than neon and can react with electron donors. each hydrogen has 2 valence electrons, the same as helium.

- the covalent bond formed between carbon and hydrogen is polar because carbon is more electronegative than hydrogen and it attracts the bonded electron pair closer to itself, thus giving hydrogen a partial positive charge.

- a hydrogen bond is a relatively weak bond that hydrogen atoms make with the electronegative atoms nitrogen, oxygen or fluorine.

so the best choice is a.) 2 calcium (ca) atoms

if you're asking what comes out, it's steam.