Asample of an unknown substance contains 38.43 g lead, 17.83 g carbon, and 3.74 g hydrogen. what is the empirical formula? a: pbc4h10 b: pb2c8h15 c: pbc8h20 d: pb2c4h15

- C: .

Solution:- An empirical formula is the simplest whole number ratio of moles of atoms.

Let's convert given grams to moles and calculate the mole ratio as:

moles of Pb =

moles of Pb = 0.1855

moles of C =

moles of C = 1.485

moles of H =

moles of H = 3.703

Let's calculate the mole ratio and for this we divide the moles of each by the least one of them. Least one is Pb as it's moles are least one.

Pb = = 1

C = = 8

H = = 20

So, the empirical formula of the compound is and the correct option is C.

The empirical formula of the unknown substance that contains 38.43 g lead, 17.83 g carbon, and 3.74 g hydrogen is PbC8H20.

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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: