A 1.00 g sample of a hydrogen peroxide (H2O2) solution is placed in an Erlenmeyer flask and diluted with 20 mL of 1 M aqueous sulfuric acid. To this solution is added 0.0200 M KMnO4 solution via a buret, until a pale purple color persists. This requires 22.50 mL of KMnO4 solution. What is the percent by mass of hydrogen peroxide in the original solution? (A) 0.613% (B) 1.53% (C) 3.83% (D) 7.65%
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Related Questions
The molar mass of carbon dioxide (CO2) is 44.01 g/mol. The molar mass of water (H2O) is 18.01 g/mol. A reaction uses 528 g of CO2. How many moles of water are used in this reaction?
If you have a crush and they are available but you don't know weather to ask them or just leave it alone which one to do
The point at which a substance is at complete equilibrium is called? User: a hydrogen bond is a special form of what type of bond
The phase of matter where particles at extremely high temperatures become ionized.
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1. (2.06g C4H10)/(58.12 g/mol C4H10) = 0.035mol C4H10
2. (0.035molC4H10)(10 mol H2O/2mol C4H10) = 0.177mol H2O
3. (0.177mol H2O)(18.01g/mol H2O) = 3.19g H2O
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To counter the removal of A the equilibrium change by shifting toward the left
explanation
If the reaction is at equilibrium and we alter the condition a new equilibrium state is created
The removal of A led to the shift of equilibrium toward the left since it led to less molecules in reactant side which favor the backward reaction.( equilibrium shift to the left)
For Plato users :
The equilibrium SHIFTS LEFT. Simultaneously, there’s an increase in the REVERSE reaction.
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Hope that helped you.
It's a physical because you have to actually do the work by using your hand to give a haircut
B. The critical temperature is the temperature above which the liquid phase of a pure substance cannot exist.
C. The critical temperature is the temperature below which the liquid phase of a pure substance cannot exist.
D. The critical temperature is the temperature at which all three phases can coexist.
E. The critical temperature is the temperature at which the pure substance reaches, but cannot go beyond, the critical pressure.
Can someone explain this one?
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After temperature reaches certain treshold the difference between density of liquid and gas state disappears, and it is impossible to liquify the substance.
Answer:what do u mean tho
Explanation:
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Answer:
The volume of the gas at 200 mmHg will be 2 L.
Explanation:
As the volume increases, the gas particles (atoms or molecules) take longer to reach the walls of the container and therefore collide with them fewer times per unit of time. This means that the pressure will be lower because it represents the frequency of collisions of the gas against the walls. In this way pressure and volume are related, determining Boyle's law which says:
"The volume occupied by a certain gaseous mass at constant temperature is inversely proportional to pressure"
Boyle's law is expressed mathematically as:
P * V = k
Now it is possible to assume that you have a certain volume of gas V1 that is at a pressure P1 at the beginning of the experiment. If you vary the volume of gas to a new value V2, then the pressure will change to P2, and it will be fulfilled:
P1 * V1 = P2 * V2
In this case:
- P1= 800 mmHg
- V1= 500 mL
- P2= 200 mmHg
- V2= ?
Replacing:
800 mmHg* 500 mL= 200 mmHg* V2
Solving:
V2= 2,000 mL= 2 L (being 1,000 mL=1 L)
The volume of the gas at 200 mmHg will be 2 L.