What is the mass in grams of #5.56 X 10^22# lead atoms?

Answer 1

Well, #6.0221xx10^23# individual lead atoms have a mass of #207.2*g#.

Thus, we calculate the quotient.

#(5.56xx10^22" atoms")/(6.022xx10^23*"atoms"*mol^-1)# #xx207.2*g*mol^-1# #=#

#"How many grams?"#

This fundamental concept of mass equivalency—that is, a mass representing a GIVEN number of atoms or molecules—is important to understand because it allows us to predict the mass of products that are likely to be observed for a given reactant. Throughout your chemistry studies, you will solve a lot of these kinds of problems.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer 2

Caleb Adams

The mass of 5.56 × 10^22 lead atoms is approximately 874 grams.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.