Write the balanced complete equation for the reaction, and then write the net io

Question

Write the balanced complete equation for the reaction, and then write the net ionic equation. Do not forget state symbols? A reaction initially contains 0.223 moles of chromium(II) sulfide and 0.652 moles of hydrochloric acid acid. When the reaction is complete, what reagent is left over, and how much of the reagent is left (in moles)? The chromium-containing product in the reaction has a molar mass of 122.8 Assume I run the reaction as described in (b) above, and I find that my percent chromium-containing product is 78%. What amount (in grams) of chromium product did I get?

Explanation / Answer

Solution :-

Balanced reaction equation is as follows

CrS(s) + 2HCl (aq) -------- > CrCl2(aq) + H2S(aq)

b) moles of CrS =0.223

moles of HCl = 0.652

mole ratio is 1 :2 for the CrS to HCl

so moles of the HCl needed to react with the CrS are calculated as

0.223 mol CrS * 2 mol HCl / 1 mol CrS = 0.446 mol HCl

So the CrS is the limiting reactant

And moles of HCl remain = 0.652 mol – 0.446 mol = 0.206 mol HCl remain

Part C ) Thereoretical moles of the CrCl2 that can be formed are 0.223 moles because mole ratio is 1 :1

Now lets calculate the moles formed using the percentage

0.223 mol CrCl2 * 78.0 % / 100 % = 0.17394 mol CrCl2

Now lets calculate its mass

Mass = moles * molar mass

Mass of product = 0.17394 mol * 122.8 g per mol

                              = 21.36 g CrCl2

So the mass of product that can be formed = 21.36 g

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