How many liters of oxygen gas can be produced at STP from the decomposition of 0

Question

How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 H,0, in the reaction according to the chemical equation shown below? 19. 2 H,02() 2 H2O() + 02(g) 20. A 1.000 kg sample of nitroglycerine, C,H,N,Og, explodes and releases gases with a temperature of 1985°C at 1.100 atm. What is the volume of gas produced? 4CHN,0g(s) 12 CO(8)+ 10 H,0(g)+6N(2)+ 02(g) The following reaction is used to generate hydrogen gas in the laboratory. If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg, what mass of hydrogen is produced? The water vapor pressure at 25°C is 23.78 mm Hg. 21. Mg(s) +2 HCl(aq) MgCl2(aq) + H2(g) Determine the volume of S0, (at STP) formed from the reaction of 96.7 g of FeS, and 55.0 L of O, (at 398 K and 1.20 atm). The molar mass of Fes, is 119.99 g/mol. 22. 4 Fe$(s) + 1 1 02(g) 2 Fe,0,6) + 8 so,(g)

Explanation / Answer

19)

no. of mole = malarity X volume of solution in liter

no. of mole of H2O2 = 3.00 X 0.250 = 0.750 mole

According to balanced chemical reaction 2 mole of H2O2 produce 1 mole of O2 then 0.750 mole of H2O2 produce

0.750/2 = 0.375 mole of O2

at STP 1 mole gas occupy volume = 22.414 liter then 0.375 mole O2 occupy volume = 22.414 X 0.75 / 1 = 8.4 L

8.4 liter O2 produced at STP

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