A molecule of ethyl alcohol is converted to acetaldehyde in one’s body by zero order kinetics. If the concentration of alcohol i
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Answer:- C = 3.024 g, H = 0.42 g, N = 1.176 g and O = 4.032 g
Solution:- The compound contains C, H, N and O. On combustion, all the carbon is converted to carbon dioxide, All hydrogen is converted to water and all the nitrogen is converted to nitrogen dioxide.
From the grams of all these, we could calculate their moles and then using mol ratio of these products and the number of moles of C, H and N present in them, we calculate the moles of C, H and N respectively. Further, these moles are converted to grams. On subtracting the sum of grams of C, H and N from the mass of the sample, the mass of oxygen is calculated.
The calculations are as follows:
Calculations for the grams of C:-
= 3.024 g C
Calculations for the grams of H:-
= 0.42 g H
Calculations for the grams of N:-
= 1.176 g N
Mass of the compound is given as 8.652 g. Now we could calculate the grams of oxygen as:
mass of oxygen = 8.652 - (3.024 + 0.42 + 1.176)
= 8.652 - 4.62
= 4.032 g
So, 8.652 grams of the compound contains 3.024 g of C, 0.42 g of H, 1.176 g of N and 4.032 g of O.
265.2 mmHg is the partial pressure of oxygen in 780 mmHg of total pressure.
Explanation:
The partial pressure of a gas is defined as the individual pressure of the gas in total mixture. In an ideal gas all the constituent gases have partial pressure some of which will give total pressure of the gas.
The partial pressure of a gas is calculated by
total pressure x mole fraction of the gas.
Mole fraction of the oxygen present is 0.34 as it is 34% of the total gas.
= 0.34 is the mole fraction
Total pressure is given as 780 mm Hg
The partial pressure can be calculated using the above formula:
Putting the values in equation:
780 x 0.34
= 265.2 mm Hg is the partial pressure of oxygen.