Hydrogen peroxide can decompose to water and oxygen by the following reaction: 2 H2O2(l) → 2...
Hydrogen peroxide can decompose to water and oxygen by the following reaction: 2 H2O2(l) → 2 H2O(l) + O2(g) ΔH = –196 kJ Calculate the value of q when 5.00 g of H2O2(l) decomposes at constant pressure.
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![2H₂ , (17 24 oll) + O₂(g) Au=-1968] Moles of H₂O x mass moler mas 5.00g 348/mol 0.147 mol - 196 kJ x 0.147 m 2 mol 14.41 KJ](http://img.homeworklib.com/questions/f37b8760-78b9-11ea-881f-673a0bd99c85.png?x-oss-process=image/resize,w_560)
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Hydrogen peroxide can decompose to water and oxygen by the
following reaction: 2 H2O2(l) → 2...
Part A Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction....
Part A Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction. 2 H2O2() + 2 H2O(1) + O2() AH =-196 kJ Calculate the value of (kJ) in this exothermic reaction when 3.00 g of hydrogen peroxide decomposes at constant pressure? -1.73 x 104 kJ -0.0289 kJ -8.65 kJ -17.3 kJ 1.92 kJ Submit Reguest Answer
Review I Constants I Per Part A Hydrogen peroxide decomposes to water and oxygen at constant...
Review I Constants I Per Part A Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: AH-196 kJ 2 H202()2 H O() +O2(g) Calculate the value of q (kJ) in this exothermic reaction when 5.00 g of hydrogen peroxide decomposes at constant pressure? -14.4 kJ -2.88 x 104 kJ 1.15 kJ -0.0173 kJ -28.8 kJ Request Answer Previous Answers Submit X Incorrect; Try Again; 4 attempts remaining N Provide Feedback
Hydrogen peroxide (H2O2) decomposes to produce water and oxygen according to the following reaction: 2 H2O2...
Hydrogen peroxide (H2O2) decomposes to produce water and oxygen according to the following reaction: 2 H2O2 (l) -----------> 2 H2O (l) + O2 (g) Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? Group of answer choices 2 molecules of H2O2 -----------------> 2 molecules of H2O + 1 molecule of O2 2 mol of H2O2 ----------------->2 mol of H2O + 1 mol of O2 68.0 g of H2O2 -----------------> 36.0 g of H2O...
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) +...
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) + 1/2 O2(g) 26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(2) + 1/2O2(g) At 20.0 °C, the half-life for the reaction is 3.05 x 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 8.00 days?
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
Hydrogen peroxide decomposes to water and oxygen: 2 H2O2 (1) + 2 H20 (1) + O2(g)...
Hydrogen peroxide decomposes to water and oxygen: 2 H2O2 (1) + 2 H20 (1) + O2(g) Which solution would have a faster rate of decomposition: A solution of 3% H2O2 or a bottle of 30% H2O2?
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
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ...
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ Part B: How many kilojoules are released when 3.05 moles of H2O2 reacts? Express your answer with the appropriate units. Part C: How many kilojoules are released when 277 g of O2 is produced? Express your answer with the appropriate units.
Hydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and...
Hydrogen peroxide can be prepared in several ways. One method is
the reaction between hydrogen and oxygen, another method is the
reaction between water and oxygen. Calculate the ?G°rxn of each
reaction below using values from this table.
(1) H2(g) + O2(g)
H2O2(l)
G =
(2) H2O(l) + 1/2O2(g)
H2O2(l) G
=
Which method requires less energy under standard conditions?
Hydrogen peroxide decomposes into water and oxygen according to the following reaction: 2H2O2(1)→ 2H2O(g) + O2(g)...
Hydrogen peroxide decomposes into water and oxygen according to the following reaction: 2H2O2(1)→ 2H2O(g) + O2(g) 0.11 g of H2O2 is decomposed in a flask with a volume of 2.50 L. What is the pressure of O2 at 298 K? a. 0.032 atm b. 0.048 atm C. 0.016 atm d. 0.16 atm e. None of the above Predict the signs of AH° and ASº for the following reaction: O2(g) + O2(1) a. + AH°; + AS° b. + AH°; -...
Part A Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction. 2 H2O2() + 2 H2O(1) + O2() AH =-196 kJ Calculate the value of (kJ) in this exothermic reaction when 3.00 g of hydrogen peroxide decomposes at constant pressure? -1.73 x 104 kJ -0.0289 kJ -8.65 kJ -17.3 kJ 1.92 kJ Submit Reguest Answer
Review I Constants I Per Part A Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: AH-196 kJ 2 H202()2 H O() +O2(g) Calculate the value of q (kJ) in this exothermic reaction when 5.00 g of hydrogen peroxide decomposes at constant pressure? -14.4 kJ -2.88 x 104 kJ 1.15 kJ -0.0173 kJ -28.8 kJ Request Answer Previous Answers Submit X Incorrect; Try Again; 4 attempts remaining N Provide Feedback
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) + 1/2 O2(g) 26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(2) + 1/2O2(g) At 20.0 °C, the half-life for the reaction is 3.05 x 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 8.00 days?
Hydrogen peroxide decomposes to water and oxygen: 2 H2O2 (1) + 2 H20 (1) + O2(g) Which solution would have a faster rate of decomposition: A solution of 3% H2O2 or a bottle of 30% H2O2?
Hydrogen peroxide can be prepared in several ways. One method is
the reaction between hydrogen and oxygen, another method is the
reaction between water and oxygen. Calculate the ?G°rxn of each
reaction below using values from this table.
(1) H2(g) + O2(g)
H2O2(l)
G =
(2) H2O(l) + 1/2O2(g)
H2O2(l) G
=
Which method requires less energy under standard conditions?
Hydrogen peroxide decomposes into water and oxygen according to the following reaction: 2H2O2(1)→ 2H2O(g) + O2(g) 0.11 g of H2O2 is decomposed in a flask with a volume of 2.50 L. What is the pressure of O2 at 298 K? a. 0.032 atm b. 0.048 atm C. 0.016 atm d. 0.16 atm e. None of the above Predict the signs of AH° and ASº for the following reaction: O2(g) + O2(1) a. + AH°; + AS° b. + AH°; -...
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