density of hydrogen peroxide
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Hydrogen peroxide ( H 2 O 2) is an oxidizer commonly used as a bleach. It is a clear liquid, slightly more viscous than water, that appears colorless in dilute solution. It is used as a disinfectant, antiseptic, oxidizer, and in rocket ry as a propellant. The oxidizing capacity of hydrogen
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Answers:30% H2O2 70% H2O Assume 1 liter of solution. If the density of the solution is 1.11g/ml, then the 1 liter of solution would have a mass of (1.11g/ml)(1000ml/L)= 1110 g 30% of 1110 g = .30 x 1110 g = 333g Molecular weight of H2O2 is 2 x 1.0 + 2 x 16.0 = 34.0 333g(1 mole/34.0g) = 9.79 moles Since you assume 1 liter, you have 9.79moles/liter Round to two significant figures. Molarity is 9.8
Answers:Physical: almost colorless, less volatile than water, denser than water, more viscous than water, miscible in water. mp: -.41 deg C bp: 150.2 deg C density: 1.6434 g/cm3 (solid at -4.5 C) 1.4425 at 25C Viscosity: 1.245 centipoise (20C) vapor pressure (@ 25C) 1.9mmHg dielectric constant: (25C) 70.7 Electric conductivity (25C) 5.1E-8 ohm^-1 cm^-1 standard heat of formation -187.6 kJ/mol standard gibbs free energy of formation: -118.0 kJ/mol Chemical: spontaneously disproportionates decomposition strongly catalyzed by metal surfaces (Platinum, Silver) can act as oxidizing or reducing agent (in both acidic and basic solutions) evolves O2 when a reducing agent can undergo proton acid/base reactions to form peroxonium salts, hydroperoxides, and peroxides somewhat stronger acid than water (pKa=11.65) much weaker base than water (by a a 10^6 factor) used in the production of epoxides, propylene oxide, and caprolactones, hydroquinone, and many pharmaceuticals and food products environmental applications include pollution treatment by oxidizing cyanides and sulfides, and restoring aerobic conditions to sewage waters. replaces chlorine in industrial bleach because H2O and O2 decomp. products That should be a start.
Answers:I1) PV = nRT n = PV/RT. I think you got it upside down. Convert P to atm, V to L, if you are using R in L atm mol-1 K-1. ALWAYS write down the units and you won't go wrong. 2) Take number of moles in (1). Double it cos q tells you to. then use molarity x volume (L) = number of moles. That should get you started.