Chemistry
From the equation:
C + 2H2SO4 ⟶ CO2 + 2H2O + 2SO2
Calculate:
(i) The mass of carbon oxidized by 49 g of sulphuric acid.
(ii) The volume of sulphur dioxide measured at STP, liberated at the same time.
Related Questions
Following questions refer to one mole of chlorine gas.
(a) What is the volume occupied by this gas at S.T.P.?
(b) What will happen to the volume of gas, if pressure is doubled?
(c) What volume will it occupy at 273°C?
(d) If the relative atomic mass of chlorine is 35.5, what will be the mass of 1 mole of chlorine gas?
(a) A hydrate of calcium sulphate CaSO4.xH2O contains 21% water of crystallisation. Find the value of x.
(b) What volume of hydrogen and oxygen measured at S.T.P. will be required to prepare 1.8 g of water.
(c) How much volume will be occupied by 2g of dry oxygen at 27°C and 740 mm pressure?
(d) What would be the mass of CO2 occupying a volume of 44 litres at 25°C and 750 mm pressure?
(e) 1 g of a mixture of sodium chloride and sodium nitrate is dissolved in water. On adding silver nitrate solution, 1.435 g of AgCl is precipitated.
AgNO3 (aq) + NaCl (aq) ⟶ AgCl (s) + NaNO3
Calculate the percentage of NaCl in the mixture.
(i) A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correct to 1 decimal place. (H = 1; C = 12; Cl = 35.5)
(ii) The relative molecular mass of this compound is 168, so what is it's molecular formula?
Find the percentage of
(a) oxygen in magnesium nitrate crystals [Mg(NO3)2.6H2O].
(b) boron in Na2B4O7.10H2O. H=1,B=11,O=16,Na=23.
(c) phosphorus in the fertilizer superphosphate Ca(H2PO4)2