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If 300g of iron pyrites is burned in 200g of O2,143 of ferric oxide is produced.What is the percentage yield of ferric oxide?
So, let's write an chemical equation:4FeS2+11O2=2Fe2O3+8SO2Let's find the amounts of substances of oxygen and iron pyrite.n(O2)=m(O2)/M(O2)=200 g/32 g/mol = 6.25 moln(FeS2)=m(FeS2)/M(FeS2)=300 g/120 g/mol = 2.5 molIron pyrite is in the...
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A fuel contains 4% hydrogen; 89% carbon; 1% sulphur; 2,5% oxygen, 3,5% ash and 20% excess air is supplies
Calculate
1.1 The mass of oxygen required to complete combustion of 1kg of fuel
1 kg of fuel contain 40 g of hydrogen, 890 g of carbon and 10 g of sulphur. 2H2 + O2 = 2H2O For complete combustion of 40 g of...
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methanol is burned in a camp stove to provide heat for cooking if 18 g of methanol is burned what will the volume of oxygen measured at 37°C and 98.8 KPA required for complete combustion
2CH3OH + 3O2 = 2CO2 + 4H2On (O2) = 3 x n (CH3OH) /2M (CH3OH) = 32.04 g/moln (CH3OH) = 18 / 32.04 = 0.56 moln (O2) = 3 x...
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What is the enthalpy change if 105 g of ethane is burned in a combustion reaction whose molar enthalpy of combustion is -1251 kJ/mol. *
n = m / MM (C2H6) = 30.07 g/moln (C2H6) = 105 / 30.07 = 3.5 moldelta H (C2H6) = - 1251 x 3.5 = -4367 kJ
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the combustion of methane produces carbon dioxide and water. assume that 2.5 mol of ch4 burned in the presence of excess air. what is the percent yield if the reaction produces 77.0g of CO2?
CH4+2O2=CO2+2H2On(CO2):n(CH4)=1:1=2.5molm(CO2)=n(CO2)*M(CO2)=2.5*44=110gȠ=(mpr/mt)*100%=(77/110)/100%=70%Answer: Ƞ=70%
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The heat of combustion of carbon in excess air is 3935 jmol-. Calculate the heat change when 60g of carbon undergoes complete combustion to produce carbon (iv) oxide ( C = 12, O = 16 )
C+O2=CO23935 x 60 /12 = 19 675 j/mol = 19,675 kj/mol.
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A 1.55 gram sample pf pentanol, C5H11OH is burned and produced a temperature increase of 55 0 C in 200 g of water. Calculate the heat of combustion of pentanol.
At first, heat absorbed by water should be calculated.Q=cm∆T, where c is a specific heat of water.Q=4.184×200×55=46024(J).It is equal (but with opposite sign) to heat released during combustion.Q=-46024 J =...
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Butane (C4H10) is burned with 35% excess air. Find the composition of the flue gas if combustion is complete.
2C4H10 + 13O2 = 8CO2 + 10H2Ofor burned 1 mol of butane, we need 6.5 mol of O2. If we have 35% excess than 1 mol of butane we waste...
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A strip of magnesium was burned according to the equation Mgist 1/202(g) → MgOis) and 40.0 kJ of heat was released to the surroundings. Calculate the mass of magnesium burned in the reaction.
2Mg + O2 = 2MgO + 1204 kJ.40 x 48/1204 = 1,59468439 g of Mg.
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