The heat change for the decomposition of 26.9 g of hydrogen peroxide (H2O2) is -145.31 kJ....
The heat change for the decomposition of 26.9 g of hydrogen peroxide (H2O2) is -145.31 kJ. What is the enthalpy of reaction (in kJ) for the process with respect to moles of hydrogen peroxide? Report your answer to 3 significant figures.
Hint: Check the sign of your answer.
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The heat change for the decomposition of 26.9 g of hydrogen
peroxide (H2O2) is -145.31 kJ....
When one mole of gaseous hydrogen peroxide, H2O2, is made from hydrogen and oxygen gases, the enthalpy change is –136 kJ...
When one mole of gaseous hydrogen peroxide, H2O2, is made from hydrogen and oxygen gases, the enthalpy change is –136 kJ. Which of the following correctly represents the thermochemical equation? i. H2(g) + O2(g) → H2O2(g) + 136 kJ ii. H2(g) + O2(g) + 136 kJ → H2O2(g) iii. H2(g) + O2(g) → H2O2(g) ΔH = –136 kJ iv. H2(g) + O2(g) → H2O2(g) ΔH = +136 kJ A.i only B.ii only C.iii only D.i and iii E.ii and iv
Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an...
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 H, O2 (1) H2(g) +O2(g) Calculate the enthalpy change using the following data: 2H2O2()2H2 O (l) + O2(g); AH = -196.0 kJ H2(g) +O2(g)H2O(); AH= -285.8 kJ ΔΗ- kJ 10 item attempts remaining Try Another Version Submit Answer
If 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined...
If 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 8.03°C was observed, The specific heat of water is 4.18 J/(g * ∘C) Calculate the enthalpy of decomposition of hydrogen peroxide (ΔH) determined from the experimental data. Record your answer with the proper significant figures and include the correct sign if needed. Assume the density and specific heat of the solution are the same as that of water.
The balanced equation for the decomposition of hydrogen peroxide, H2O2, is given below. What number of...
The balanced equation for the decomposition of hydrogen peroxide, H2O2, is given below. What number of grams of O2 result from 3 . g of hydrogen peroxide? 300. g O2 3. g O2 320. g O2 338. g O2
In a study of the gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)----->H2O(g) +...
In a study of the gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)----->H2O(g) + ½ O2(g) the concentration of H2O2 was followed as a function of time. It was found that a graph of 1/[H2O2] versus time in seconds gave a straight line with a slope of 0.884 M-1 s-1 and a y-intercept of 7.04 M-1. Based on this plot, the reaction is _______zerofirstsecond order in H2O2 and the rate constant for the reaction is M-1 s-1.
I recently conducted an experiment looking at the enthalpy change in a decomposition reaction of hydrogen...
I recently conducted an experiment looking at the enthalpy change in a decomposition reaction of hydrogen peroxide using a catalyst (Iron (III) chloride) and am now writing a report for it. The literature states that the change in enthalpy for this reaction should be 94.6 kJ mol-1 (exothermically), whereas our experimentation determined the enthalpy change to be 100.7 kJ mol-1. In the discussion section, I am discussing how the calorimeter used would not create a 'perfect' environment and would still...
The first-order decomposition of hydrogen peroxide has a half-life of 10.7 h at 20°C. a. What...
The first-order decomposition of hydrogen peroxide has a half-life of 10.7 h at 20°C. a. What is the rate constant (expressed in hr−1) for this reaction? _____________ Write answer to three significant figures and NO UNITS in answer. b. If you started with a solution that was 7.5 × 10−3 M H2O2, what would be the concentration of H2O2 after 3.3 h? __________
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)->H2O(1) + 12 02(g)...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)->H2O(1) + 12 02(g) is first order in H2O2- During one experiment it was found that when the initial concentration of 1,0, was 3.16x10-2 M, the concentration of H2O2 dropped to 8.09x10-3 M after 945 min had passed. Based on this experiment, the rate constant for the reaction is nin-1
3. The decomposition of gaseous hydrogen peroxide to O2(g) and H2O(g) is a first-order reaction. Experimentally,...
3. The decomposition of gaseous hydrogen peroxide to O2(g) and H2O(g) is a first-order reaction. Experimentally, at a given temperature, the initial concentration of H2O2 was found to decease to one- half in 17.0 minutes. What fraction of the initial H2O2 would remain after 51 minutes?
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g)...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3 min-1. If the initial concentration of H2O2 is 5.66×10-2 M, the concentration of H2O2 will be 9.34×10-3 M after _______ min have passed.
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 H, O2 (1) H2(g) +O2(g) Calculate the enthalpy change using the following data: 2H2O2()2H2 O (l) + O2(g); AH = -196.0 kJ H2(g) +O2(g)H2O(); AH= -285.8 kJ ΔΗ- kJ 10 item attempts remaining Try Another Version Submit Answer
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)->H2O(1) + 12 02(g) is first order in H2O2- During one experiment it was found that when the initial concentration of 1,0, was 3.16x10-2 M, the concentration of H2O2 dropped to 8.09x10-3 M after 945 min had passed. Based on this experiment, the rate constant for the reaction is nin-1
3. The decomposition of gaseous hydrogen peroxide to O2(g) and H2O(g) is a first-order reaction. Experimentally, at a given temperature, the initial concentration of H2O2 was found to decease to one- half in 17.0 minutes. What fraction of the initial H2O2 would remain after 51 minutes?
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