How do you balance #Fe(s) + S(s) - Fe_2S_3(s)#?

Question

How do you balance #Fe(s) + S(s) -> Fe_2S_3(s)#?

Ellie Andrews · Accepted Answer

#2Fe_(s)# + #3S_(s)# ------------> #Fe_2S_3#

Step 1 : First of all write the equation #Fe_(s)# + #S_(s)# ------------> #Fe_2S_3#

Step 2 : Now balance the number of #Fe# atoms on both reactant and product side

Here reactant side has one #Fe_(S)# atom and product side has #2# atoms of #Fe_(S)#, therefore multiply #Fe_(S)# at reactant side by #2#

Step 3: Balance #S_(s)#

Here reactant side has one #S_(s)# atom and product side has #3# atoms of #S_(s)#, therefore multiply #S_(s)# at reactant side by #3#

Step 4: Compose the last equation.

#2Fe_(s)# + #3S_(s)# ------------> #Fe_2S_3#

Cameron Andrews · Answer

undefined To balance the equation Fe(s) + S(s) -> Fe2S3(s), you need to ensure that the number of atoms of each element is the same on both sides of the equation. Start by counting the number of Fe atoms and S atoms on each side of the equation. Then adjust the coefficients to balance the equation. In this case, you would need to put a coefficient of 4 in front of Fe(s) and a coefficient of 3 in front of S(s) to balance the equation. So, the balanced equation would be: 4Fe(s) + 3S(s) -> Fe2S3(s).

How do you balance #Fe(s) + S(s) -&gt; Fe_2S_3(s)#?

How do you balance #Fe(s) + S(s) -> Fe_2S_3(s)#?