The limiting reactant in the reaction would be the compound that would be consumed completely in the reaction. The balanced chemical reaction for this problem is written as:
<span>MnO2 + 4HCl → MnCl2 + 2H2O + Cl2
From the reaction and the amounts present of the reactant, the limiting reactant would be HCl or hydrochloric acid. Ten moles of HCl only need 2.5 moles of MnO2. Hope this helps.</span>
Answer:
Explanation:
The volume and amount of gas are constant, so we can use Gay-Lussac’s Law:
At constant volume, the pressure exerted by a gas is directly proportional to its temperature.
Data:
p₁ =5.7 atm; T₁ = 100.0 °C
p₂ = ?; T₂ = 20.0 °C
Calculations:
1. Convert the temperatures to kelvins
T₁ = (100.0 + 273.15) K = 373.15
T₂ = (20.0 + 273.15) K = 293.15
2. Calculate the new pressure
Answer:
'Oxidation states have changed.'
Explanation:
Redox Reactions can be identifiable by a change in oxidation number/states of two of the atoms in the reaction. Any reaction in which no oxidation numbers/state change is not a redox reaction.
Gas to solid ( a ) is correct i think
Answer: 4) Concentrate it
Explanation: