Hydrogen consumption in hydrochloric acid production
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Our company produces 196 tons of 31% hydrochloric acid per day, with a chlorine purity of 80%. There is a significant difference between the value calculated theoretically and the flow rate indicated by the actual hydrogen flow meter – what could be the reason for this? How should the hydrogen consumption be calculated?
In actual production, an excess of hydrogen is required; I wonder what excess amount you used in your calculations? Measure the exhaust emissions to see what the actual excess value is Sometimes, the values displayed on the instrument may not be very accurate, resulting in overestimations or underestimations that require correction.
This post was last edited by qugd on 2016-11-30 09:53. Why is the purity of this chlorine so low? Is it the chlorine from the chlor-alkali plant? Theoretically, when synthesizing hydrochloric acid, the volumes of chlorine and hydrogen consumed are equal. However, in practice, a slight excess of hydrogen is used, at a ratio of about 5–10% by volume. Pay strict attention to whether the impurities in chlorine contain oxygen; if oxygen is present, it is necessary to strictly control the temperature of the material entering the absorption tower, as water is generated, and a low temperature upon entry into the absorption tower can cause severe corrosion.
The minimum purity required for the production of synthetic chlorine is 65%, while that for hydrogen should be above 98%; generally, the ratio of chlorine to hydrogen is 1:1.05–1.1
Our theoretical calculation for the amount of hydrogen required is (chlorine purity + 2 * oxygen content) * 1.05–1.1; 2 volumes of hydrogen are needed for every 1 volume of oxygen consumed. If the oxygen content is high, in order to ensure that the hydrochloric acid reaches top-quality standards, the ratio of hydrogen to oxygen may end up being above 1.15.
Is the chlorine used in the OP’s home to produce liquid chlorine the same kind of chlorine?
Is the chlorine used by the poster’s family waste chlorine from the liquid chlorine production process?
”Our theoretical calculation for the amount of hydrogen required is (chlorine purity + 2 * oxygen content) * 1.05–1.1; 2 volumes of hydrogen are needed for every 1 volume of oxygen consumed. If the oxygen content is high, in order to ensure that the hydrochloric acid reaches top-quality standards, the ratio of hydrogen to oxygen may end up being above 1.15. “ This explanation is quite reasonable; please check what gases are present in the other 20% of the components
With such low chlorine purity, it must be waste chlorine that has been liquefied. Another 20% is estimated to be nitrogen and hydrogen. Be careful with nitric chloride; it’s very dangerous.
The formation of nitric chloride must occur during the electrolysis process; it shouldn’t have anything to do with liquid chlorine, right?