# A 3.4g sample of h2o2 solution containing x% H2O2 by mass requires x ml of a KMnO4 solution for complete oxidation under acidic condition. The molarity of KMnO4 solution is: a)1 b)0.5 c)0.4 d)0.2

66,417 results
1. ## Chemistry

Calculate Delte G Knot for H20(g) + 1/2 O2 H2O2(g) at 600. K, using the following data: H2(g) + O2(g) H2O2 (g) K = 2.3 X 10^6 at 600. K 2H2(g) + O2(g) 2H20(g) K= 1.8 X 10^37 at 600. K

2. ## Science

Hydrogen peroxide, H2O2, is unstable under certain conditions and decomposes as follows: 2 H2O2 â†’ 2 H2O + O2 ? g 34.00 g 15.98 g What mass of hydrogen peroxide, to the nearest hundredth of a gram, is decomposed in this reaction? Please help ðŸ˜”

3. ## Chemistry

The formaldehyde content of a pesticide preparation was determined by weighing 0.3124g of the liquid sample into a flask containing 50.0mL of 0.0996M NaOH and 50mL of 3% H2O2. Upon heating, the following reaction took place: OH- + HCHO + H2O2 -> HCOO- +

4. ## chemistry

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition. 2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ How much heat is released when 529 kg H2O2 decomposes? ( ......... ) KJ *note ..watch sig figs . my

5. ## chemistry

When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)âŸ¶2H2O(l)+O2(g)Î”H=âˆ’196kJ How many kilojoules are released when 2.65 moles of H2O2 reacts? How many kilojoules are released when 234 g of O2 is produced?

6. ## Chemistry

Enthalpy changes: H2O2(l) ----> H2O(l) + 1/2P2(g) delta H= -94.6kJ H2(g) + 1/2O2(g)----> H2O2 delta H= -286.0kJ Calculate the value on delta H for the reaction: H2(g) + H2O2(l)----> 2H2O(l)

7. ## Chemistry

Hydrogen peroxide can act as either an oxidizing agent or a reducing agent, depending on the species present in solution. Write balanced half-reaction equations for each of the following: (a) H2O2(aq) acting as an oxidizing agent in an acidic solution.

8. ## Chemistry

A galvanic cell is based on the following half-reactions at 25C: Ag+ + e- --> Ag H2O2 + 2H+ + 2e- ---> 2H2O (not H2O2) Predict whether E_cell is larger or smaller than EÂ°_cell for the following case. [Ag+]= 1.0M, [H2O2]= 2.0 M, [H+]=2.0M

9. ## Biology

What are the roles of hydrogen peroxide, oxygen, hydrogen, and catalase in the following chemical reaction? catalase 2H2O2 > O2 + 2H2O A. Catalase is an enzyme, O2 and H2O are substrates, and H2O2 is a reactant. B. Catalase is a substrate, O2 and H2O are

10. ## Chemistry

Calculate Delta G for H2O(g) + 1/2 O2(g) H2O2(g) at 600. K using the following data: H2(g) + O2(g) H2O2(g) k = 2.3 X 10^6 at 600. K 2H2(g) + O2(g) 2H2O(g) k = 1.8 X 10^37 at 600. K

11. ## chemistry

Hydrogen peroxide, H2O2, is used to disinfect contact lenses. What volume of O2, in mL, or O2(g) at 31 degree celsius, and 741mmHg can be liberated from 10.0mL of an aqueous solution containing 3.00% H2O2 by mass? The density of aqueous solution of H2O2 is

12. ## Chemistry

Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2O2 can be prepared in a process whose overall change is the following. H2(g) + O2(g) H2O2(l) Calculate the enthalpy change using the following data.

13. ## Science

15.2% by mass solution of h2o2, density is 1.01g/ml then find the molarity of the sulution.

Write the standard line notation for each cell below. IO3-(aq) + Fe2+(aq)--> Fe3+(aq) +I2(aq) ________________________________________ H2O2 + 2 H+ + 2 e- --> 2 H2O E = 1.78 V O2 + 2 H+ + 2 e- --> H2O2 E= 0.68 V ________________________________________ Mn2+

15. ## Chemistry

A 3.4g sample of h2o2 solution containing x% H2O2 by mass requires x ml of a KMnO4 solution for complete oxidation under acidic condition. The molarity of KMnO4 solution is: a)1 b)0.5 c)0.4 d)0.2

16. ## science---1 question

help pls asap! 2) Which of the following is a pure substance? (1point) Chocolate milk Orange juice Seawater Hydrogen peroxide (H2O2) i first thought it was C (seawater) but is it D (H2O2)!??

17. ## chemistry; kinetics

Use the following table to determine the average rate during the period 800 to 1200 seconds for the decomposition of H2O2. 2 H2O2(l) â†’ 2 H2O(l) + O2(g) Time (sec) (H2O2)M 0 2.32 400 1.72 800 1.30 1200 0.98 1600 0.73 a] 1.2 x 10-3M/sec b] 1.6 x 10-3 M/sec

18. ## Chem

A 3.4g sample of h2o2 solution containing x% H2O2 by mass requires x ml of a KMnO4 solution for complete oxidation under acidic condition. the molarity of kmno4 solution is: a)1 b)0.5 c)0.4 d)0.2

19. ## Chemistry

The decomposition of hydrogen peroxide is first order in H2O2: 2H2O2(aq) â†’ 2H2O(l) + O2(g) Rate = k [H2O2] How long will it take for half of the H2O2 in a 10-gal sample to be consumed if the rate constant for this reaction is 5.6 x 10-2 s-1?

20. ## science

20ml solution containing 0.2g of an impure sample of h2o2 reacts with 0.316g of kmno4 in the presence of h2so4. Find the purity of h2o2 in the mixture.

21. ## science

drogen peroxide, H2O2, is unstable under certain conditions and decomposes as follows: 2 H2O2 â†’ 2 H2O + O2 ? g 34.00 g 15.98 g What mass of hydrogen peroxide, to the nearest hundredth of a gram, is decomposed in this reaction?

22. ## Chemistry

A half-life of a H2O2 solution at a certain condition is 4 weeks. You have a 100 mL of 1.00M H2O2 solution. How many moles of H2O2 will be left in the solution after the following weeks? 04 weeks after: moles 08 weeks after: moles 16 weeks after: moles 20

23. ## Science

Nitric oxide reacts hydrogen to give nitrogen and water(2no+2h2_n2+2h2o).the kinetics of this rxn is explained byfollowing zteps:(1)2no+h2_n2+h2o2(slow)( 2) h2o2+h2_2h2o(fast).

24. ## Chemistry

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

25. ## Chemistry

Hydrogen peroxide, H2O2, solution can be purchased in drug stores and used as an antiseptic. A sample of such a solution weighing 1.00 grams was acidified with sulfuric acid and titrated with .02000 M solution of KMnO4. The unbalanced reaction is H2O2(aq)

26. ## Chemistry

A solution contains H2O2 in water. Complete decomposition of the H2O2 in 170 g of this solution yields 5.6 L of O2(g), measured at 0 oC and 101.325 kPa. What is the percentage by mass of H2O2 in this solution? Choose the closest answer. A 10% B 20% C 5.0%

27. ## AP Chem

A solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4. It requires 51.7 mL of 0.145 M KMnO4 to titrate 20.0 g of the solution of hydrogen peroxide. What is the mass percentage of H2O2 in the solution? If you

28. ## Chemistry

if antiseptic hydrogen peroxide is 3% H2O2 by mass, approximately how many moles of H2O2 are present in each gram of antiseptic solution? you can assume the solution has the same density as water. show your calculations.

29. ## chem

I need help balancing this redox equation: H2O2 + Ni+2 --> H2O + Ni+3 in basic solution. Here's what I have so far: Ni+2 --> Ni+3 + 1e- H2O2 --> H2O I can't seem to make the second half-reaction balance. If you follow the rules for balancing basic redox

30. ## Chemistry

1)How many mL of H2O2 are in 969 mL in solution ? * Given: 5.0% of H2O2 by volume. 2)What is the mole fraction of the solute in a 1.35m solution of CaCl2?

31. ## chemistry

A mixture of hydrogen peroxide, H2O2, and hydrazine, N2H4, can be used as a rocket propellant. The reaction is: 7 H2O2(g) + N2H4(l) Â® 2 HNO3(aq) + 8 H2O(l) a) How many moles of H2O2 react with 0.477 mol N2H4? [1] ___________ b) How many grams of HNO3 can

32. ## Chemistry

I am so confused with my chemistry lab right now. We were given the following equations to work with: [Equation 1] 2 I^- + H2O2 + 2 H^+ ----> I2 + 2 H2O [Equation 9] 2S2O3^2- + I2 ----> 2I^- +S4O6^2- And During the Experiment we used the following for each

33. ## chemistry

can u help me in this question. The rate of appearance of I2 in aqueous solution, in the reaction of I^- ion with hydrogen peroxide, was found to be 3.7*10^-5 mol. L^-1.s^-1 over time interval. 2H^+(aq)+ 2I^-(aq)+H2O2-> I2(aq)+2H2O(l) During the same

34. ## chemistry

The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data. H2O2 + I - = H2O + IO - (slow) H2O2 + IO - = H2O + O2 + I - (fast) Which

35. ## why will no one answer? chem

The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data. H2O2 + I - = H2O + IO - (slow) H2O2 + IO - = H2O + O2 + I - (fast) Which

36. ## chem

In a solution at constant H+ concentration, iodide ions react with hydrogen peroxide to produce iodine. H+ + I- + 1/2H2O2 --> 1/2I2(aq) + H2O The reaction rate can be followed by monitoring the appearance of I2. The following data were obtained:

37. ## chemistry

hello, I am trying to find an answer for cooling H2O2 in synthesis of hexaamminecobalt(III) chloride but did not cooled H2O2 for the synthesize pentaamminechlorocobalt(III) chloride..

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism: step 1 slow: H2O2 + I^- = H2O + OI^- step 2 fast: H2O2 + OI^- = H2O + O2 + I^- 1) What is the equation for the overall reaction? Use

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism: step 1 slow: H2O2 + I^- = H2O + OI^- step 2 fast: H2O2 + OI^- = H2O + O2 + I^- 1) What is the equation for the overall reaction? Use

40. ## Chemistry

A 2.00 ml sample of an aqueous solution of hydrogen peroxide, H2O2 (aq) is treated with an excess of Kl (aq). The liberated I2 requires 12.40 mL of 0.1025 M Na2S2O3, for its titration. Is the H2O2 up to the full strength (3% H2O2 by mass) as an antiseptic

A 2.00 ml sample of an aqueous solution of hydrogen peroxide, H2O2 (aq) is treated with an excess of Kl (aq). The liberated I2 requires 12.40 mL of 0.1025 M Na2S2O3, for its titration. Is the H2O2 up to the full strength (3% H2O2 by mass) as an antiseptic

A 2.00 ml sample of an aqueous solution of hydrogen peroxide, H2O2 (aq) is treated with an excess of Kl (aq). The liberated I2 requires 12.40 mL of 0.1025 M Na2S2O3, for its titration. Is the H2O2 up to the full strength (3% H2O2 by mass) as an antiseptic

43. ## Chemistry

A 3.4g sample of h2o2 solution containing x% H2O2 by mass requires x ml of a KMnO4 solution for complete oxidation under acidic condition. The molarity of KMnO4 solution is: a)1 b)0.5 c)0.4 d)0.2

44. ## Science

A 3.4g sample of h2o2 solution containing x% H2O2 by mass requires x ml of a KMnO4 solution for complete oxidation under acidic condition. the molarity of kmno4 solution is: a)1 b)0.5 c)0.4 d)0.2

45. ## lab

Number of moles of oxygen gas produced from the complete catalyzed decomposition of 6.80ml sample of a 3.5% solution. Density of the 3.5% solution of H2O2 is 1.01g/ml Let's find out what you know about this and work from there. Show your calculations to

46. ## Chemistry

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

47. ## Chemistry

A solution of hydrogen peroxide, H2O2, is titrated with potassium permanganate, KMnO4, according to the following equation: 5H2O2 + 2KMnO4 + 3H2SO4 = 5O2 + 2MnSO4 + 8H2O + K2SO4. It requires 46.0 mL of 0.145 Mol/L KMnO4 to titrate 50.0 mL of the solution

48. ## Chemistry

A solution of hydrogen peroxide, H2O2, is titrated with potassium permanganate, KMnO4, according to the following equation: 5H2O2 + 2KMnO4 + 3H2SO4 = 5O2 + 2MnSO4 + 8H2O + K2SO4. It requires 46.0 mL of 0.145 Mol/L KMnO4 to titrate 50.0 mL of the solution

49. ## chemistry

a 500.0 g sample of h2o2 conatins 31.50% h2o2 by mass find the mass of water in the solution

50. ## College Chemistry

The density of a 0.0122 M KMnO4 is 1.037 g/mL. Suppose 26.35 g of 0.0122 M KMnO4 are required to titrate 1.072 g of a household H2O2 solution. a)Calculate the mL of MnO4^- added to reach the endpoint. b)Calculate the moles of MnO4^- added to reach the

51. ## Chemistry 30

predict the products of the reaction between acidified H2O2 with potassium permanganate solution H2O2 (l) ïƒ  KMnO4 (aq) + 2H2O (l) + 6H+ (aq) + 6e- H2O2 (l) + 2H2O (l) ïƒ  KMnO4 (aq) + + 6H+ (aq) + 6e- is this right? I'm confused. May I please get help?

52. ## chemistry

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition. 2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ How much heat is released when 529 kg H2O2 decomposes? ( ......... ) KJ *note ..watch sig figs . my

53. ## chemistry

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition. 2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ How much heat is released when 529 kg H2O2 decomposes? ( ......... ) KJ *note ..watch sig figs . my

54. ## chemistry

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition. 2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ How much heat is released when 529 kg H2O2 decomposes? ( ......... ) KJ *note ..watch sig figs . my

55. ## chemistry

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition. 2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ How much heat is released when 529 kg H2O2 decomposes? ( ......... ) KJ *note ..watch sig figs . my

56. ## Biology

For my Biology Lab I have to create a graph showing my results. We used an enzyme, and put in a substrate (H2O2). Every 10, 30, 60, 90, 120, 180, and 360 second H2O2 was killed with acid. To measure the amount of H2O2 we used KMnO4. Now to the question. I

57. ## Chemistry

In the reaction between H2O2 and I-, 15 mL of 0.30M KI, 65. mL of 0.10M H2O2 and 19 mL of 0.020M Na2S2O3 were mixed in a flask containing starch and buffer and the total volume was made up to 500mL with distilled water. The solution turned blue (indicating

58. ## chemistry

consider the balanced chemical equation 2H2O2 ---> 2H2) + )O2 A) given 20.0 g of H2O2 how many grams of water will be produced? B) how many grams of H2O2 will you need to get 20.0 g of water ? C) how many grams of H2O2 will you need to get 20.0 g of O2 D)

59. ## Chemistry

The density of hydrogen peroxide, H2O2, is 1.45 g/mL. How many molecules of H2O2 are in 0.350 L of hydrogen peroxide? The molar mass of H2O2 is 34.01 g/mol.

60. ## CHEM

Hydrogen peroxide (H2O2) is decomposed according to the following reaction: 2H2O2 (l) Â¡Ã· 2H2O (l) + O2 (g) If 6.00 g of aquesous solution containing hydrogen peroxide was decomposed after heating, the mass of oxygen gas collected is 2.40 g, what is the

61. ## chemistry

i had a lab that combined 1/2 cup of H2O2 (118.3 ml) and 2 tsp of yeast. is the equation for the reaction 2H2O --> 2H2O + O2 what would the mass be for each product in the reation? Is the density of H2O2 1.4g/ml? Here is some interesting reading on this

62. ## chemistry

What is the mass of hydrogen peroxide, H2O2, in a 250 g sample of a 2.75% by weight solution?

63. ## Chemistry

In the reaction 2H2O2(aq)-->2H2O2 + O2 (g), There is intially 0.865 M H2O2. After 10.0 minutes, the molarity of H2O2 changes to 0.792 M. What is the rate of reaction in terms of H2O2?

64. ## Chemistry

If all the H2O2 in 25mL of a 3% solution of H2O2 decomposed, calculate the diameter of a sphere that would contain the resulting O2 at 1 atm and 296K. I understand how to do the problem if I have moles but I am not sure how to get moles. I thought

65. ## Chemistry

Using the set of smallest possible integer coefficients to balance the redox equation H2O2 +MnOâˆ’4 -> O2 +Mn+2 (acidic solution), the coefficient for H2O2 is 1. 5. 2. The correct coefficient is not given. 3. 2. 4. 7. 5. 4.

66. ## chem

2H202--> 2H20 +O2 Given that you started with Â½ cup of H2O2, what was the mass of each product in the reaction? (1/2 cup = 118.3 mL, density of H2O2 is 1.4 g/mL)

67. ## Chemistry

Iron (II) ion is oxidized by hydrogen peroxide in acidic solution. H2O2(aq) + 2Fe2+(aq) + 2H+(aq) ---> 2Fe3+(aq) + 2H2O (l) the rate law is k[H2O2][Fe2+] what is the order with respect to each reactant ? what is the overall order

68. ## Organic Chemistry

A half-life of a H2O2 solution at a certain condition is 4 weeks. You have a 100 mL of 1.00M H2O2 solution. How many moles of H2O2 will be left in the solution after the following weeks? 04 weeks after: moles 08 weeks after: moles 16 weeks after: moles 20

69. ## chem-redox

write down Oxidation equation, Reduction equation and Overall equation theres 3 equations *H2O2 + H2SO4 + KMnO4 *H2O2 + KMnO4 *and *Ethanol + H2O2 + K2Cr2O7

70. ## chemistry-help!

The initial rate of reaction for H2O2(aq) H2O (l) 1/2 O2 (g) is found to be 1.7x10(-3)M/s. Assume that this rate holds for 2 minutes. Start with 160ml of 1.60 M H2O2. How many milliliters of O2 measured at 24C and 760mmHg , are released from solution in

71. ## Chemistry

The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data. H2O2 + I - = H2O + IO - (slow) H2O2 + IO - = H2O + O2 + I - (fast) Which

72. ## Chemistry

Use the concentrations and volumes of hydrogen peroxide and KI before mixing (Table 1), calculate the post-mixing concentrations. Before mixing: [H2O2] = 0.88M [KI] = 0.500M Table 1: before mixing 1. Vol H2O2 = 4.0 mL, [H2O2] = 0.88M 2. Vol KI = 1.0 mL,

73. ## chemistry

The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data. H2O2 + I - = H2O + IO - (slow) H2O2 + IO - = H2O + O2 + I - (fast) Which

74. ## chemistry

The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data. H2O2 + I - = H2O + IO - (slow) H2O2 + IO - = H2O + O2 + I - (fast) Which

75. ## chemistry

How do i calculate the concentration of H2O2 after 150 mL of distilled water is added to 30 mL of 1.0 M of H2O2?

76. ## chemistry

calculate the molarity of H2O2 if 25ml of H2O2 required 12 ml of 0.1M KMN04? The right answer 0.24M who helps

77. ## Chemistry

Thank you for your help. I did want to clarify why you are only calculating the Molar Mass for H2 and not the molar mass for H2O (or even H2O2). I'm not sure why you did this. Please clarify. See below: The following reaction represents the decomposition

78. ## Chem

I'm having a lot of trouble with a simple problem. I have a 3.0% by man solution of H2O2 in H2O. The density of thr solution is 1.0 g/mL. I need to find the molarity. How do I do this? So far I have: 3.0g H2O2 x 1 mol/34.02 g= .0881 mol I'm not sure where

79. ## Chemistry

Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide,H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the

80. ## science

the decomposition of h2o2 is first order reation following up the decom position it was found that the remaining h2o2 after 45 min was 15 units from the original concentration57.5 unit calculate the rate constant

81. ## Chemistry

Hi can someone please help with this question, or atlest direct me in the right direction. Please and thank you. The initial rate of reaction H2O2(aq) --> H2O (l) + 1/2 O2(g) is found to be1.7*10^-3 M/s . Assume that this rate holds for 2 minutes. Start

82. ## chemistry_toughhhh

Initial rate of rxn of H2O2(aq)->H2O+ 1/2 O2(g) is found at 1.7x10(-3)M/s and is constant for 2min. You start with 160ml of 16M H2O2. How many mL of O2 in one minute? (Measured at 273K and 760mmHg). I tried to find the new conc of H2O2 via NewConc= Old

83. ## chemistry

Which of the following rate laws suggests that the reaction probably occurs in a single step? why is this problem cant be answer a since it has order of 1 a)(CH3)3CBr + OH- â†’(CH3)3COH + Br- rate = k[(CH3)3CBr] b)NO(g) + O2(g) â†’ NO2(g) + O(g) rate =

84. ## chemistry

Which of the following rate laws suggests that the reaction probably occurs in a single step? why is this problem cant be answer a since it has order of 1 a)(CH3)3CBr + OH- â†’(CH3)3COH + Br- rate = k[(CH3)3CBr] b)NO(g) + O2(g) â†’ NO2(g) + O(g) rate =

85. ## chemistry

Hydorgen peroxide may be prepared by the following reactions: 2NH4HSO4 ---> H2+(NH4)2S2O8 (NH4)2S2O8+2H2O ----> 2NH4HSo4+H2O2 What mass of ammonium hydrogen sulfate, Nh4HSo4 is initially required to prepare 2.00 mole of H2O2? What mass of H2O is required?

86. ## Chemistry

Which of the following rate laws suggests that the reaction probably occurs in a single step? NO(g) + O2(g) â†’ NO2(g) + O(g) rate = k[NO][O2] H2O2 + 3 I- + 2 H+â†’ I3- + 2 H2O rate= kl[H2O2][I-]+K2[H2O2][I-][H+] H2(g) + Br2(g) â†’ 2 HBr(g) rate =

87. ## chemistry

What mass percent of a solution with 28.5 g of H2O2 and 300.0 mL of water?

88. ## Chemistry

hrdrogen peroxide, H2O2, can be placed on open wounds as in an antiseptic. When you do this, bubbling occurs because 2H2O-------> 2H2O + O2 However, H2O2 only decomposes slowly in the bottle. Why does the wound accelerate its decompostion

89. ## chemistry HELP!!

Reaction Rate = -(1/2) [d(H2O2)/dt] = [d(O2)/ dt] Using 25 mL of a 0.2 M hydrogen peroxide solution, the following results are obtained from the equation above: 8.62 mL of gas is collected in 120 seconds. (Assume 760 Torr = 1 atm) Room temperature is 25

90. ## Chemistry

How would I calculate the mass of 20ml of a 3% hydrogen peroxide from a 30% H2O2 solution?

91. ## Physics

what is the mass of hydrogen peroixide, H2O2, in 350 grams ofa 20% by weight solution?

92. ## Chem-Repost

it wouldn't let me post after putting spaces in the url and everything, so i just copied and pasted the q instead :P sorry for all the messyness. i'll see if i can delete q's, in the mean time you can maybe look at this please? Initial rate of rxn of

93. ## chemistry

hello, I am trying to find an answer for cooling H2O2 in synthesis of hexaamminecobalt(III) chloride but did not cooled H2O2 for the synthesize pentaamminechlorocobalt(III) chloride..

94. ## chemistry

Calculate the number of moles of H2O2 required to produce 0.08 moles of HNO3 by the following reaction. 7 H2O2 + N2H4 2 HNO3 + 8 H2O

95. ## Chemistry

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism: step 1 slow: H2O2 + I^- = H2O + OI^- step 2 fast: H2O2 + OI^- = H2O + O2 + I^- 1) What is the equation for the overall reaction? Use

96. ## Chemistry

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism: step 1 slow: H2O2 + I^- = H2O + OI^- step 2 fast: H2O2 + OI^- = H2O + O2 + I^- 1) What is the equation for the overall reaction? Use

97. ## Chemistry

The catalysed decomposition of H2O2 in aqueous solution is followed by titrating equal volume of sample solutions with KMnO4 solution at different time interval give the following results. Show that the reaction is a first order reaction. t (mins) 0 5 15

98. ## Chemistry

Another proposed mechanism problem: H2O2 + I ---> H2O +IO slow H2O2 + IO ---> H2O + O2 + I fast Which of the following statements in incorrect? a.) IO is a catalyst b.) I is a catalyst c.) The net reaction is 2H2O2 ---> 2H2O + O2 I would choose B, since IO

99. ## chemistry

From a hydrogen peroxide (diluted in water) a sample of 1.00 g is removed, acidifing it with H2SO4 and then titrated with a solution of 0.20 M of KMnO4, requiring 17.6 mL of KMnOH. What is the percentage of H2O2 contained in the bottle?