1) If 5 litres of H2O2 produce 50 lites of O2 at NTP, H2O2 is
a)50V
b)10V
c)5V
d)250V
I am not able to understand this question. What is it asking?
2)Assuming that petrol is octane & has density 0.8 g/ml, 1.425 litres of petrol on complete combustion will consume how many moles of oxygen?
3)10ml of gaseous hydrocarbon on ombustion gives 40ml of CO2(g) & 50ml of H2O(vap). The hydrocarbon is ?????
4)5.5 g of a mixture of FeSO4.7H2O and Fe2(SO4)3.9H2O requires 5.4ml of 0.1N KMnO4 solution for complete oxidation. Calculate the numbers of moles of hydrated ferric sulphate in the mixture.
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1 Answers
11Q2
given density and volume are 0.8g/ml and 1.425L=1425mL
therefore given mass of petrol=0.8*1425g=1140g
moles of petrol= 1140/114=10
the chemical equation of combustion of octane is:
2C8H18 + 25O2 → 8Co2 + 9H2O
25moles of O2 react with 2 moles octane
therefore with 10 moles of octane no of moles of oxygen = 25*10/2
ans = 125
Q3 Is the answer butane(C4H10) ??
