Question

What is the percent of hydrogen peroxide in the solution when 5.02g of H2O2 solution reacts...

What is the percent of hydrogen peroxide in the solution when 5.02g of H2O2 solution reacts to produce 0.153g of H2O? 2H2O2 (l) → 2H2O (l) + O2 (g)

Mass percent = (mass of solute/mass of solution)*100

a) 3%

b) 5%

c) 30%

d) 50%

(if your answer doesn't match one of the choices, that's probably because there was a typo in the original question, and I fixed it to make sense. it was: "...5.02g of H2O2 solution reacts to produce 0.153g of H2O2?..." which didn't make very much sense.)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
If hydrogen peroxide H2O2 decomposes according to the equation: 2H2O2 → 2H2O + O2                      ∆H =...
If hydrogen peroxide H2O2 decomposes according to the equation: 2H2O2 → 2H2O + O2                      ∆H = −196 kJ Calculate the heat evolved on decomposition of 5g of H2O2.
Given the decomposition of hydrogen peroxide, calculate the moles of oxygen gas produced from 4.20 mol...
Given the decomposition of hydrogen peroxide, calculate the moles of oxygen gas produced from 4.20 mol of H2O2. 2H2O2(l)→2H2O(l)+O2(g)
Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated...
Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated by light, heat, or a catalyst. The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from 12.9 g of a 7.50% hydrogen peroxide solution?
QUESTION 6 The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H2O2(aq) -->...
QUESTION 6 The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H2O2(aq) --> 2 H2O(l) + O2(g) Using data from a concentration-time study of this reaction, which plot will produce a straight line? [H2O2] versus time [H2O2]2 versus time 1 / [H2O2] versus time ln[H2O2] versus time
A solution of hydrogen peroxide, H2O2 , is titrated with potassium permanganate, KMnO4 , according to...
A solution of hydrogen peroxide, H2O2 , is titrated with potassium permanganate, KMnO4 , according to the following equation: 5 H2O2 + 2 KMnO4+ 3H2SO4 -> 5O2 + 2 MnSO4 +8H2O + K2SO4 It requires 46.9mL of 0.145 mol/L KMnO4 to titrate 50.0 mL of the solution of H2O2 . What is the moles per litre concentration of H2O2 in the solution?
Consider the decomposition of hydrogen peroxide to form water and oxygen, 2H2O2(g) ⇋ 2H2O(g) + O2(g)...
Consider the decomposition of hydrogen peroxide to form water and oxygen, 2H2O2(g) ⇋ 2H2O(g) + O2(g) A researcher places 2.86 moles of H2O2 in a volume of 5.50L at 307 ℃. After equilibrium was reached, 2.00 moles of H2O2 remained. Reactants and products → [H2O2] [H2O] [O2] Initial Change Equilibrium Use the information given to fill out the ICE table above. Each box must be completed. Determine the equilibrium concentration of each component of the reaction. Using the values from...
Hydrogen peroxide, H2O2, can act as both an oxidising agent or a reducing agent according to...
Hydrogen peroxide, H2O2, can act as both an oxidising agent or a reducing agent according to the following half reactions: Oxidising agent: H2O2(aq) + 2H+(aq) +2e– → 2H2O(l) Reducing agent: H2O2(aq) → O2(g) + 2H+(aq) 2e– What simple visual cue would indicate a reaction where H2O2 is acting as a reducing agent? formation of water increase in pH appearance of electrons bubbles of gas
2) The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in...
2) The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in 13.2−g of hair bleach was determined by titration with a standard potassium permanganate solution: 2 MnO4−(aq) + 5 H2O2(aq) + 6 H+(aq) → 5 O2(g) + 2 Mn2+(aq) + 8 H2O(l) (a) For the titration, how many moles of MnO4− were required if 32.3 mL of 0.195 M KMnO4 was needed to reach the end point? Write your answer to the correct number of...
Reaction 6: Decomposition of Hydrogen Peroxide with Potassium Iodide 2 H2O2 (aq) + 2 I -...
Reaction 6: Decomposition of Hydrogen Peroxide with Potassium Iodide 2 H2O2 (aq) + 2 I - (aq) ---> 2 H2O (l) + O2 (g) + I2 (aq) (simplified reaction) 1. Place 2 to 3 mL of hydrogen peroxide (H2O2) into a clean and dry test tube. Record observations. 2. Drop a single pellet of potassium iodide into this test tube. Over the next 2 minutes, record observations regarding any changes observed. 6 Clear solution, thicker After drop a potassium iodide,...
The activation energy for the decomposition of hydrogen peroxide is 55.0 kJ/mol. When the reaction is...
The activation energy for the decomposition of hydrogen peroxide is 55.0 kJ/mol. When the reaction is catalyzed by the enzyme catalase, it is 11.00 kJ/mol. 2H2O2(aq) → 2H2O(l) + O2(g) Calculate the temperature that would cause the nonenzymatic catalysis to proceed as rapidly as the enzyme-catalyzed decomposition at 20.0°C. Assume the frequency factor, A, to be the same in both cases. Report your answer to 3 significant figures.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT