In the following reaction, how many atoms of Sn would be produced if we start with 4.0 moles of H2? SnO2 + 2 H2 → Sn + 2 H2O

1.02x10^24 atoms

Explanation:

The coefficients (the numbers before each susbtance) in this equation tell us that for every 2 moles of hydrogen used, there will be 1 mole of tin produced. This is a fixed ratio, which means if we use 4 moles of H2, 2 moles of tin will be produced.

One mole contains Avogadro's number of atoms (6.02 x 10^23). So two moles would contain twice as many atoms as this.

2 x 6.02x10^23 = 1.02x10^24 atoms.

:)

1.2044  x 10^24 atoms

Explanation:

The equation of the reaction is given as;

SnO2 + 2 H2 → Sn + 2 H2O

From the reaction;

2 ml of H2 produces 1 mol of Sn

4 mol of H2 would produce x mol

2 = 1

4 = x

Solving for x;

2x = 4

x = 4 /2 = 2 mol

The relationship between mol and atoms is given as;

1 mol = 6.022 × 10 23 atoms

2 mol = x

x = 2  * 6.022 × 10^23

x = 12.044 x 10^23 = 1.2044  x 10^24 atoms

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation: