Chemistry Questions Attached are 8 questions that I’m really struggling with. They cover Stoichiometry, limiting reactions, determining chemical formulas,
Chemistry Questions Attached are 8 questions that I’m really struggling with. They cover Stoichiometry, limiting reactions, determining chemical formulas, and analysis of a mixture. Please help me with this, I’m really struggling. I need the answers by 11:45pm MST tonight. If you can’t explain the answers to me within that time frame thats totally okay, I just need the answers. But please explain them to me after you give me the answers. There is no time limit on the explanations, but the answers I need in 2 hours. According to the following reaction, how many grams of ethane (C2H) will be formed upon the complete reaction of 23.8 grams of
ethylene (C2H4) with excess hydrogen gas ?
hydrogen(g) + ethylene (C2H4)(g)
ethane (C2H)(g)
grams ethane (C2H6)
According to the following reaction, how many grams of chlorine gas are required for the complete reaction of 32.9 grams of iron ?
iron(s) + chlorine(g)
iron(III) chloride(s)
grams chlorine gas
Identify limiting reactants (mole ratio method).
Identify the limiting reactant in the reaction of iron and oxygen to form FeO, if 19.2 g of Fe and 9.52 g of O2 are combined. Determine the amount (in grams) of
excess reactant that remains after the reaction is complete.
Formula of limiting reactant
Amount of excess reactant remaining
=
g
Identify limiting reactants (maximum product method).
Consider the reaction of diboron trioxide with carbon and chlorine.
B203 (s) + 3C (s) + 3Cl2 (g)
→2BC13 (g) + 3CO (g)
Determine the limiting reactant in a mixture containing 190 g of B203, 117 g of C, and 488 g of Cl2. Calculate the maximum mass (in grams) of boron trichloride,
BC13, that can be produced in the reaction.
The limiting reactant is:
B203
ОС
Cl2
Amount of BC1z formed
g
Use combustion analysis to determine empirical and molecular formulas (hydrocarbons).
Furnace
02
H20 absorber
CO2 absorber
Sample
When 4.647 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 13.60 grams of CO2 and 8.355 grams of H20 were produced.
In a separate experiment, the molar mass of the compound was found to be 30.07 g/mol. Determine the empirical formula and the molecular formula of the
hydrocarbon.
Enter the elements in the order presented in the question.
empirical formula
molecular formula
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