You allow 4.78g of A and 10g of B to react to form C. Assuming you had a perfect reaction, how many grams of B would be leftover at the end of the reaction? A + 2B -> C

A = 202.0g/mole
B = 85.0 g/mole
C = 105 g/mole

If someone could send me the steps on how to solve this, that would be extremely helpful.

About 8 gallons of fuel will be used. (8.08)

Given data,temperature, t = 230°c = 503 kconsider the chemical reaction,ch₃oh(l) + 1/2 o₂(g)  → ch₂o(g) + h₂o(l)calculate the enthalpy change for the reaction: δh⁰rxn =  σnδh⁰f(products) -  σmδh⁰f(reactants)substitute the values from the table: δh⁰rxn = { -115.9 + (-285.8)} - {0+(-238.7)}              = -163.0 kjcalculate the entropy change for the reaction.δs⁰rxn = (219 + 70) - (127.2 + 1/2 x 205.2) = 59.2 j/kconsider the expression for free energy: δg⁰rxn =  δh⁰rxn - t  δs⁰rxnsubstitute the values in the above equationδg⁰rxn = -163 x 10³ - (503 x 59.2)              = -192777.6 j              = -192.777 kj