Question

An iron atom has a mass of 9.27(10)^-23 g and a cooking pot

Answer 1

Complete Question:

An iron atom has a mass of 9.27*(10)⁻²³ g and a cooking pot has a mass of 0.500 kg.

Use this information to answer the questions below:

1) What is the mass of 1 mole of iron atoms? Round your answer to 3 significant digits.

The mass of 1 mole of iron atoms is 55.8 g

Why?

The key to solve this question is the use of the Avogadro's Number (NA). This number tells us the amount of atoms found in 1 mole of a substance. So, to find the mass of 1 mole of iron atoms, we're actually finding the mass of 6.022 x 10²³ atoms.

The equation we are going to use to find the mass is shown below:

$mass_{1moleFe}=mass_{1atomFe}*NA=(9.27*10^{-23}g/atom)* (6.022*10^{23})\\\\mass_{1moleFe}=55.8 g$

2) How many moles of iron atoms have a mass equal to the mass of a cooking pot? Round your answer to 3 significant digits.

The moles of iron atoms that have a mass equal to the mass of a cooking pot is 8.96 moles

Why?

In this case, we are also going to use the mass of the cooking pot. We have to find first how many atoms are there in the cooking pot, and then we will find how many moles are represented by that mole of atoms:

Atoms in the cooking pot:

$\# atoms=0.500kg*\frac{1000g}{1kg}*\frac{1 atom}{9.27*10^{-23} } =5.39*10^{24}atoms$

Moles in the cooking pot:

$\# moles=5.39*10^{24}atoms*\frac{1 moles}{6.022*10^{23}atoms } =8.96 moles$

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