What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm3 flask at 27 °C ?
Given,
Mass of carbon dioxide = 4.4 g
Molar mass of carbon dioxide= 44g/mol
Mass of methane = 3.2g
Molar mass of methane = 16g/mol
Now amount of methane, nCH4 = 3.2/ 16 = 0.2 mol
& amount of CO2 nCO2 = 4.4/ 44 = 0.1 mol
Also we know ,
Pv = (nCH4 + nCO2) RT
OR P X 9 = (0.2 +0.1) x 0.0821 x 300
Or p = 0.3 x 0.0821 x 300 / 9 = 0.821 atm
Hence, the total pressure exerted by the mixture is 0.821 atm
The mass of an electron is 9.1 × 10–31 kg. If its K.E. is 3.0 × 10–25 J, calculate its wavelength.
Calculate the amount of carbon dioxide that could be produced when
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(iii) 2 moles of carbon are burnt in 16 g of dioxygen.
Calculate the wavelength of an electron moving with a velocity of 2.05 × 107 ms–1.
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(b) MnO4 – (aq) + SO2 (g) → Mn2+ (aq) + HSO4– (aq) (in acidic solution)
(c) H2O2 (aq) + Fe 2+ (aq) → Fe3+ (aq) + H2O (l) (in acidic solution)
(d) Cr2O7 2– + SO2(g) → Cr3+ (aq) + SO42– (aq) (in acidic solution)
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(ii) 2 mol A + 3 mol B
(iii) 100 atoms of A + 100 molecules of B
(iv) 5 mol A + 2.5 mol B
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(c) energy of quantum and
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