A.) How many grams of phosphorus react with 35.5L of O2 at STP to form tetraphos

Question

A.) How many grams of phosphorus react with 35.5L of O2 at STP to form tetraphosphorus oxide, according to the following reaction equation?

P4(s)+5O2(g)--> P4O10(s)

B.) Ammonia decomposes to nitrogen and hydrogen when in the presence of heated steel whool. what is the final volume of the gas when 45g of ammonia decomposes at 150`C and 1atm pressure. write a balanced equation before you start your calculations!

2B) ammonia is completely decomposed to nitrogen and hydrogen, as in question B). At the end of the experiment the pressure of gas mixture is 866mmHg. calculate the partial pressures of N2 and H2.

Dalton's law of partial pressure

A.) earth's atmosphere consist of 78% N2 and 20% O2 and other gases. what is the partial pressure of N2 and O2 in torr, when the atmospheric pressure is1atm?

Explanation / Answer

A)At STP ( pressure = 1 atm and T = 273 K) the volume of one mole of gas is 22.4 L

moles O2 = 35.5 / 22.4 =1.58

the ratio between P4 and O2 is 1 : 5

moles P4 required = 1.58/5=0.316

molar mass P4 = 4 x 30.9738 g/mol=123.895 g/mol

mass P4 = 0.316 mol x 123.895 g/mol=39.2 g

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