Answer:
the answer is mabye 30 I didnt understand
Answer:
Please see the complete formt of the question below
Chlorine gas can be made from the reaction of manganese dioxide with hydrochloric acid.
MnO₂(s) + HCl(aq) → MnCl₂(aq) + H₂O(l) + Cl₂(g)
According to the above reaction, determine the limiting reactant when 5.6 moles of MnO₂ are reacted with 7.5 moles of HCl.
The answer to the above question is
The limiting reactant is the MnO₂
Explanation:
To solve this, we note that one mole of MnO₂ reacts with one mole of HCl to produce one mole of MnCl₂, one mole of H₂O and one mole of Cl₂
Molar mass of MnO₂ = 86.9368 g/mol
Molar mass of HCl = 36.46 g/mol
From the stoichiometry of the reaction, 5.6 moles of MnO₂ will react with 5.6 moles of HCl to produce 5.6 moles of H₂O and 5.6 moles of Cl₂
However there are 7.5 moles of HCL therefore there will be an extra 7.5-5.6 or 1.9 moles of HCl remaining when the reaction is completed
P1V1=P2V2
(600/760)(.200)=(780/760)x
x=.1538L or 153.8mL
Answer:
Activation energy for the uncatalyzed reverse reaction = 103 kJ/mol
Explanation:
Activation energy decreases from = 56 kj/mol to 35 kj/mol
products = 78 KJ lower in energy than reactants
Activation energy for the uncatalyzed reverse reaction = 103 kJ/mol
attached below are the sketches of approximate energy-level for both catalyzed and uncatalyzed reactions
