Question

__Na3PO4 + __Sr(NO3)2 --> ___Sr3(PO4)2 + __NaNO3

If .0789 moles of Strontium Nitrate are reacted, how many moles of Sodium Phosphate were reacted?

Answer 1

To find the number of moles of Sodium Phosphate reacted when 0.0789 moles of Strontium Nitrate are reacted, divide 0.0789 by 3.

Step-by-step explanation:

To find the number of moles of Sodium Phosphate reacted, we can use the balanced chemical equation:

Na3PO4 + 3Sr(NO3)2 → Sr3(PO4)2 + 3NaNO3

We can see that for every 3 moles of Sr(NO3)2 reacted, 1 mole of Na3PO4 is reacted. So if we have 0.0789 moles of Sr(NO3)2, we will have (0.0789 / 3) moles of Na3PO4 reacted.

Therefore, the number of moles of Sodium Phosphate reacted is approximately 0.0263 moles.

Answer 2

0.0526mol

Step-by-step explanation:

The chemical equation given in this equation is as follows:

Na3PO4 + Sr(NO3)2 → Sr3(PO4)2 + NaNO3

However, this equation is unbalanced as the number of atoms of each element on each side does not correlate. The balanced equation is as follows:

2Na3PO4 + 3Sr(NO3)2 → Sr3(PO4)2 + 6NaNO3

This balanced equation means that:

2 moles of Sodium Phosphate (Na3PO4) is required to react with 3 moles of Strontium Nitrate (Sr(NO3)2)

Hence, if 0.0789 moles of Strontium Nitrate are reacted, then 0.0789 × 2/3

moles of sodium phosphate will also react.

= 0.0789 × 2/3

= 0.1578/3

= 0.0526mol