Question

How many grams of silver/IN dichromate are neiled)when 353 p of Tin 1 hydrogen carbonate is complailyused up in a double displacement reaction? Use the following balanced equation:1 Sn(HCO3)2 + 1 Ag›Cr207 ---> 1 SnCr207 + 2 AgHCO3

Answer 1

`63.63\text{ g}`

Step-by-step explanation:

Here, we want to get the mass of silver(I) dichromate needed

Firstly, we need to get the number of moles of Tin(I) Hydrogen Carbonate used up

To get this, we have to divide the mass used up, by the molar mass

The molar mass of Tin(I) Hydrogen Carbonate is 241 g/mol

Mathematically:

`Number\text{ of moles = }\frac{mass}{molar\text{ mass}}`

We have the number of moles as:

`Number\text{ of moles = }(35.5)/(241)\text{ = 0.1473 mole}`

From the equation of reaction, 1 mole of Tin hydrogen carbonate used 1 mole of silver dichromate

That means 0.1473 mole of the carbonate will also use 0.1473 mole of the dichromate

Now, to get the mass of the dichromate, we have to multiply the number of moles by the molar mass of the dichromate

The molar mass of the dichromate is 432 g/mol

Thus, we have the mass used up as:

`0.1473\text{ }*\text{ 432 = 63.6 g}`