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.
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) ??
