Chemistry
The equation for the burning of octane is :
2C8H18 + 25O2 ⟶ 16CO2 + 18H2O
(i) How many moles of carbon dioxide are produced when one mole of octane burns ?
(ii) What volume, at s.t.p., is occupied by the number of moles determined in (i) ?
(iii) If the relative molecular mass of carbon dioxide is 44, what is the mass of carbon dioxide produced by burning two moles of octane ?
Related Questions
The volumes of gases A, B, C and D are in the ratio, 1 : 2 : 2 : 4 under the same conditions of temp. and press.
(i) Which sample contains the maximum no. of molecules. If the temp, and pressure of gas A are kept constant, what will happen to the volume of A when the no. of molecules is doubled.
(ii) If the volume of 'A' is 5.6 dm3 at s.t.p., calculate the no. of molecules in the actual vol. of 'D' at s.t.p. [Avog no. is 6 × 1023).
Using your answer, state the mass of 'D' if the gas is N2O
[N = 14, O = 16]
Calculate the no. of moles and the no. of molecules present in 1.4 g of ethylene gas (C2H4). What is the vol. occupied by the same amount of C2H4. State the vapour density of C2H4.
(Avog. No. = 6 × 1023 ; C = 12, H = 1]
Define the term Mole.
A gas cylinder contains 24 × 1024 molecules of nitrogen gas. If Avogadro's number is 6 × 1023 and the relative atomic mass of nitrogen is 14, calculate :
(i) Mass of nitrogen gas in the cylinder.
(ii) Volume of nitrogen at STP in dm3
A certain gas 'X' occupies a volume of 100 cm3 at S.T.P and weighs 0.5 g. Find it's relative molecular mass.