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26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) +...
peroxide decomposes into water and oxygen in a first-order process. 9. Hydrogen H:02(aq) H1/2 04g) At 20.0 °C, the half-life for the reaction is 3.92 x 10 seconds. If the initial concentration of hydrogen perox what is the concentration after 7.00 days? a. 1.2× 10-s M 0.52 M, b. 0.034 M c. 0.074 M d. 0.22 M e. 0.52 M 178
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 (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...
K= 1.54day-1
Hydrogen peroxide is used to disinfect porous surfaces like N95 masks by heating the liquid to 100C to make a vapor. Hydrogen peroxide liquid is stored as a 3.0% w/w solution at room temperature, but it quickly decomposes into water and oxygen in a first-order process. H2O2(aq) + H2O(l) + 1/2 O2(g) 4) If the initial concentration of Hydrogen peroxide is 0.52 M, what is the H2O2 concentration after 7.00 days? Use the equation In (X/Xf=kt a) 0.000012...
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
Hydrogen peroxide is made by white blood cells to destroy harmful bacteria. When hydrogen peroxide decomposes, it forms molecular oxygen and water. 2 H2O2(aq) ⟶ O2(g) + 2 H2O(g) Suppose O2 is being formed at a rate of 0.65 M/min. At what rate (M/min) is the concentration of hydrogen peroxide changing? Enter your answer to 2 decimal places.
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.
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 1.10×10-3min-1. If the initial concentration of H2O2 is 5.52×10-2 M, the concentration of H2O2 will be 1.56×10-2 M after _____ min have passed.
Over time, hydrogen peroxide, H2O2, degrades into water and oxygen gas. A bottle of hydrogen peroxide is expired and you need to determine the concentration. A titration is performed using the following equation: 3 H2O2(aq) + 2 NaMnO4(aq) → 3 O2(g) + 2 MnO2(aq) + 2 NaOH(aq) + 2 H2O(l) Note that permanganate ion, MnO4-, is purple, while manganese (IV) ion, Mn4+, is colorless. A quantity of 683 mL of 3.44 M NaMnO4 was measured and placed in a beaker. The solution...
The reaction of hydrogen peroxide with iodine, H2O2(aq)+I2(aq)?OH?(aq)+HIO(aq) is first order in H2O2 and first order in I2 . If the concentration of H2O2 was increased by half and the concentration of I2 was quadrupled, by what factor would the reaction rate increase?