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Lena772
 one year ago
Calculate the theoretical mass (in grams) of Sodium Sulfate produced using only the volume and molarity of Sulfuric Acid.
Calculate the theoretical mass (in grams) of Sodium Sulfate produced using only the mass of Sodium Carbonate.
What is the theoretical yield (in grams) of Sodium Sulfate?
What mass (in grams) of the excess reactant is left over after the reaction?
Lena772
 one year ago
Calculate the theoretical mass (in grams) of Sodium Sulfate produced using only the volume and molarity of Sulfuric Acid. Calculate the theoretical mass (in grams) of Sodium Sulfate produced using only the mass of Sodium Carbonate. What is the theoretical yield (in grams) of Sodium Sulfate? What mass (in grams) of the excess reactant is left over after the reaction?

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Lena772
 one year ago
Best ResponseYou've already chosen the best response.0\[H_{2}SO_{4}+Na_{2}CO_{3} \rightarrow H_{2}CO_{3} + Na_{2}SO_{4}\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Alright this is molarity question

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0First off this is a double displacement question and I assume you know it.

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0M= moles solute/L of solution moles solute= M*L m=4.9M*0.00698L =0.034202*105.99 g/ 1 mol = 3.6 mol However, I get that this is incorrect

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0That should say 3.6g not mol.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0This is a very simple question. You ask your periodic table "hey what's up man tell me what your molar mass label has to say and I'll add them up happy to the kingdom come"

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Oh shiz I didn't note "using only the mass for the reactant" ok

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0You do the happy stoichometry

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0Do you see where I went wrong?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Why don't you just use the stoichiometry ratio?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I recommend stoichoimetry for the sake of simplicity because it's easier

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@Nnesha what's your take on this?

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0I don't know what you mean by the stoichiometry ratio.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I am gonna give you the kingdom come so the ratio between sulfuric acid used and sodium sulfate used is 1:1 meaning that every mole of sulfuric acid results in one mole of sodium sulfate. So find the overall gram of sodium sulfate by looking at periodic table and add them together.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0for 1 mole of reactant results in 1 mole of product.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0pretty simple isn't it?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@empty if you could elaborate what I mean that's great

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0that dude got scared off

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ok I am here with you no worries

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0but I am really sleepy right now vote on my thread

Lena772
 one year ago
Best ResponseYou've already chosen the best response.0Add what together? I don't understand.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@empty pitch in dude don't be the spectator ion
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