0.01 mole of an organic compound (X) containing 10\% hydrogen, on complete combustion produced 0.9 g H2O. Molar mass of (X) is g mol-1.
100
0.9 g H2O = 0.05 mol ⇒ H = 0.1 mol = 0.1 g (in 0.01 mol of X)
This is 10\% of the sample ⇒ mass of 0.01 mol X = 1 g
M= 10.01=100 g/mol
Answer: 100
When 81.0 g of aluminium is allowed to react with 128.0 g of oxygen gas, the mass of aluminium oxide produced in grams is . (Nearest integer) Given : Molar mass of Al is 27.0 g mol-1 Molar mass of O is 16.0 g mol-1
Some CO2 gas was kept in a sealed container at a pressure of 1 atm and at 273 K. This entire amount of CO2 gas was later passed through an aqueous solution of Ca(OH)2. The excess unreacted Ca(OH)2 was later neutralized with 0.1 M of 40 mL HCl. If the volume of the sealed container of CO2 was x, then x is cm3 (nearest integer). [Given : The entire amount of CO2(g) reacted with exactly half the initial amount of Ca(OH)2 present in the aqueous solution.]
20 mL of 2 M NaOH solution is added to 400 mL of 0.5 M NaOH solution. The final concentration of the solution is 10-2 M. (Nearest integer)
The candela is the luminous intensity, in a given direction, of a source that emits monochromatic radiation of frequency 'A' 1012 hertz and that has a radiant intensity in that direction of 1'B' watt per steradian. 'A' and 'B' are respectively
Combustion of glucose ( C6H12O6) produces CO2 and water. The amount of oxygen (in g) required for the complete combustion of 900 g of glucose is : [Molar mass of glucose in g mol-1 = 180]
The density of 'x' M solution ('x' molar) of NaOH is 1.12 g mL-1, while in molality, the concentration of the solution is 3 m ( 3 molal). Then x is (Given : Molar mass of NaOH is 40 g/mol)
Molality (m) of 3M aqueous solution of NaCl is : (Given : Density of solution = 1.25 g mL-1, Molar mass in g mol-1 : Na - 23, Cl - 35.5)
The incorrect postulates of the Dalton's atomic theory are : Choose the correct answer from the options given below :
An organic compound has 42.1\% carbon, 6.4\% hydrogen and the remainder is oxygen. If its molecular weight is 342, then its molecular formula is :
The number of moles of methane required to produce 11 g CO2(g) after complete combustion is : (Given molar mass of methane in g mol-1 : 16)