Question

Balance this equation (step by step please)

Answer 1

`K_(2)CrO_(4) + Pb(NO_(3))_(2) >> 2 KNO_(3) + PbCrO_(4)`

Reactions:

`K_(2)CrO_(4) + Pb(NO_(3))_(2) >> KNO_(3) + PbCrO_(4)`

Step-by-step explanation:

In the reaction, the CrO4(Chromate) is a compound NO3(Nitrate) is a compound as well.

Ignore the number in front of the reaction first, calculate how many K, Cr, O, Pb and N in the equation for both left and right side.

Left side: K=2, Cr=1, Pb=1, N=2, O=10

Right side: K=1, Cr=1, Pb=1, N=1, O=7

So we need 3 more oxygen, 1 more nitrogen and 1 more potassium on the right.

If we add a 2 in front of KNO3, there will be 2 potassium, 2 Nitrogen and 6 oxygen, which the reaction complete.

Conclusion:

`K_(2)CrO_(4) + Pb(NO_(3))_(2) >> 2 KNO_(3) + PbCrO_(4)`