17.6 cm3 of a pure vapour, at 1.153 atm, and 98.5 °C has a mass of 0.0520 g. Calculate the molar mass of the substance.

Give detailed Solution....don't give Handwritten answer

One of the most recognizable corrosion reactions is the rusting of iron. Rust is caused by iron reacting with oxygen gas in the presence of water to create an oxide layer. Iron can form several different oxides, each having its own unique color. Red rust is caused by the formation of iron(III) oxide trihydrate. Fe,O, • 3 H,O Write the balanced reaction for the formation of Fe, O, • 3 H,O(s). Phases are optional. reaction: Fe + 6H,O + 30, Fe(OH)3 > Incorrect

This reaction is an example of conjugate addition of a nucleophile to an a,ß-unsaturated carbonyl. LOCH3 H20 H3C H3C° OCH3 OCH3 Draw the two resonance structures of the enolate anion intermediate for this reaction.

Establish the phase equilibrium for nonreacting systems in terms of the specific Gibbs function of the phases of a pure substance

contains 0.550 bar H2(g)0.550 bar H2(g) , 0.491 bar N2(g)0.491 bar N2(g) , and 0.121 bar Ar(g)0.121 bar Ar(g) . Calculate the mole fraction, ?χ , of each of these gases.

18a

A 13.5-LL scuba diving tank contains a helium-oxygen (heliox) mixture made up of 24.8 gg of HeHe and 4.40 gg of O2O2 at 298 KK. Calculate the mole fraction of each component in the mixture.

The equilibrium vapor pressure of liquid hydrogen at 16 K is 0.213 bar. The standard (1 bar) boiling point is 20.3 K. Use the Clausius-Clapeyron equation to estimate the enthalpy of vaporization of hydrogen.