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When a solution of hydrogen peroxide (H2O2) is put on a cut, bubbles, producing water and oxygen gas according to the following equation:
2H2O2 (aq) ---> 2H2O (l) + O2 (g)
If someone puts 0.570mL of a 3.00% hydrogen peroxide solution on a cut, how many moles of hydrogen peroxide are used? Assume the density of the solution is equal to the density of water.
What compounds react with the diazonium salt to give the phenolic product? Why should an excess of nitrogen be avoided in this reaction?
What is the partial pressure of SO2(g) in the larger container. What is the partial pressure of N2(g) in this vessel. What is the total pressure in the vessel
a solution initially 0.100 m in hocl and 0.300 m in naocl. what is the ph in 0.030 mol of solid naoh is added to 1.00 l
According to NMR spectra rules, a carbon that is more substituted is more deshielded. For some reason I cannot understand this, because in my mind I see it has more shielding since there is more electron density around it. Please explain in detail..
How many L of solvent should be added to 0.46 L of a 0.28 M solution if you want a final concentration of 0.13 M.
calculate the ph after 0.020 mol hcl is added to 1.00 l of each of the four solutions.a 0.100 m honh2 kb 1.1
The mass percentage of iodine in the compound was determined by converting the iodine in a 0.850 g sample of the compound into 2.31 g of lead(II) iodide. What is the empirical formula of the compound? Could the compound also contain oxygen?
what is the mole fraction of ethanol in an aqueous solution that is 46 percent ethanol by mass?
bynbsp solving this problemnbsp student cannbsp find limiting as well as excess reactant and also amount of product
Consider a 0.53 M solution of each of the following salts in distilled water. Will the solution be acidic, neutral, or basic? You may need to reference a table of Ka and Kb Tables values
calculate the composition of the vapor (in terms of mole fractions) at 25°C. At 25°C, the vapor pressures of pure CH2Cl2 and pure CH2Br2 are 133 and 11.4 torr, respectively.
A gas mixture contains oxygen and carbon dioxide. The partial pressure of oxygen is 0.450 atm. The partial pressure of carbon dioxide is 675 mm Hg. If argon gas added to the mixture causes the total pressure to become 2410 torr,
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