Created by StemPy LabMethanal, , and glucose, , have the same empirical formula, . Each is burnt completely in excess oxygen to carbon dioxide and water. Atomic masses in : H 1, C 12, O 16. Statement I: Burning of methanal and of glucose gives the same number of moles of carbon dioxide. Statement II: Burning of methanal and of glucose gives the same mass of carbon dioxide, each.
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← Natural boron is a mixture of two isotopes, with atomic masses 10.01 u and 11.01 u. Its average atomic mass is 10.81 u. A chemist weighs out 10.81 g of natural boron for a tracer experiment, in which she must know how many atoms of each isotope are present. Take NA = 6.022 × 10²³ mol⁻¹. How many atoms of the lighter isotope does this sample contain?Match each observation in List-I with the law in List-II. List-I (Observation) A. Magnesium burns in a sealed flask; the total mass is unchanged B. Black copper oxide from two sources: 1.59 g gives 1.27 g of copper, 0.795 g gives 0.635 g C. 1.00 g of sulfur takes 1.00 g of oxygen in one oxide, 1.50 g in another D. 10 mL of N₂ and 10 mL of O₂ give 20 mL of NO, at one temperature and pressure List-II (Law) I. Multiple proportions II. Conservation of mass III. Gay Lussac's law of gaseous volumes IV. Definite proportions →
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