Vijay kept staring at the door even after Jndhar had left the room.
He was lost in thought, now that his ambition for Southeast Asia had be crystal clear, he was wondering how he could use the rebels in the Indonesian archipgo and whether they would still cooperate with the Bharatiya Empire as before. It wasn’t until a servant entered the room with a beverage that he woke up from his stupor.
"Well, I guess I will take the matter one step at a time. If worstes to worst, we can just use force," Vijay decided in his mind.
Drinking the hot milk, he returned to the work he was doing before the meeting with Jndhar.
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Ever since Vijay had set goals for the researchers of the empire a month ago, the research had never stopped, even with the Ganesha Chaturthi celebrations in the middle.
Vijay frequently reviewed the projects of different research groups and what they were working on along with their progress. Even among the research goals, Vijay was mainly paying attention to the research and development tasks of three acids and two bases.
He wasn’t too worried about the research tasks he had assigned for the development of new machine tools; the Bharatiya Empire had rich experience in this field, so he did not have to worry.
The chemical industry was a new field for the empire, so it required his constant attention. Currently, Vijay is looking at the experimental logs of a few research groups that looked promising.
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R&D Team #46, Experimental Log: Arjun Patel to Mass Production Sulfuric Acid
Researcher: Arjun Patel, Chief Chemist, Bharatiya Acadamy of Military Sciences
Assistant Researcher: Bhaskar Iyer, Bharatiya Acadamy of Civilian Sciences
Medical Factory Consultant: Rajani Deshmukh
Helpers from the University: Kavita Mehra, Pranav Chandra, Raghav Nair
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Log Entry: August 14, 1657
Objective: Develop arge-scale production method for a strong acid suitable for medical and industrial uses.
Today’s Experiment: Attempted to produce acid by burning sulfur (S) in arge y pot, allowing the fumes to pass over metal tes. The reaction used was:
S+O2?→SO2?
The sulfur dioxide (SO?) was intended to be absorbed by the water to form sulfurous acid:
SO2?+H2?O→H2?SO3?
However, only a faint, weak liquid formed, and most of the fumes escaped.
Failure Analysis: The setup was too open; fumes were not contained effectively. Metal tes corroded quickly, resulting in weak and impure acid.
Next Steps: Construct a more closed environment to contain fumes better and use materials that won’t corrode.
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Log Entry: August 24, 1657
Objective: Improve the containment of sulfur fumes and increase acid yield.
Today’s Experiment: Built a sealed iron chamber to contain the sulfur fumes. Burned sulfur inside and directed the fumes into a water bath. The reaction setup was:
S+O2?→SO2?
SO2?+H2?O→H2?SO3?
Despite this, the iron corroded rapidly, and the water bath failed to capture sufficient fumes.
Failure Analysis: Iron was unsuitable due to rapid corrosion. The water bath did not efficiently absorb the fumes into a strong acid.
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Next Steps: Use less reactive materials for the chamber and enhance the absorption process.
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R&D Team #264, Experimental Log: Ravi Sharma to Mass Produce Hydrochloric Acid
Researcher: Ravi Sharma, Lead Chemist, Bharatiya Academy of Civilian Sciences
Assistant Researcher: Manoj Verma, Chemist, Bharatiya Academy of Civilian Sciences
Helpers from the University: Deepa Rao, Nikhil Joshi, Le Agarwal
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Log Entry: August 14, 1657
Objective: Develop a method forrge-scale production of hydrochloric acid.
Experiment: Began by attempting to produce hydrochloric acid (HCl) using the reaction betweenmon salt (sodium chloride, NaCl) and sulfuric acid (H?SO?, Lab produced). Heated the salt in arge y pot and added sulfuric acid, expecting the reaction to produce hydrogen chloride gas (HCl), which would then dissolve in water to form hydrochloric acid. The reaction is represented as:
NaCl+H2?SO4?→NaHSO4?+HCl(g)
Fumes of HCl gas were released, but the acid collected was very diluted, and the process was messy, with fumes escaping and posing a hazard.
Failure Analysis: The reaction produced excessive heat, causing rapid evaporation of the acid, leading to significant gas loss. The apparatus was also difficult to control and unsafe.
Next Steps: Design a more controlled apparatus to capture and condense the gas.
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Log Entry: August 19, 1657
Objective: Improve gas containment and acid concentration.
Experiment: Constructed a closed system using ss tubes to direct the HCl gas from the NaCl and H?SO? reaction into a cooling chamber. A water trap was added to absorb the gas and form hydrochloric acid:
HCl(g)+H2?O→HCl(aq)
Manoj suggested increasing the cooling surface area to enhance gas condensation. However, the ss tubes cracked under pressure, and only a small amount of weak acid was collected. The gas flow was erratic and uneven.
Failure Analysis: Corrosion contaminated the product, and the cooling method was inadequate.
Next Steps: Use non-reactive materials for the pipes and enhance gas condensation.
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R&D Team #411, Experimental Log: Vikram Singh Mass Production of Calcium Hydroxide
Researcher: Vikram Singh, Chemist, BIT Nasik
Assistant Researcher: Nem Patel, BIT Jagdalpur
Lab Helpers: Arjun Desai, Rajiv Mehta, Sunita Rao
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Log Entry: August 14, 1657
Objective: Develop a method forrge-scale production of calcium hydroxide (ked lime).
Today’s Experiment: Attempted to produce calcium hydroxide by directly reacting calcium carbonate (CaCO?) with water. The reactions were:
CaCO3?+H2?O→Ca(OH)2?+CO2?
Failure Analysis: The reaction was inefficient, with much of the calcium carbonate remaining unreacted. The setup did not adequately handle therge quantities of material, resulting in a low yield of calcium hydroxide. The process was too slow and ineffective.
Next Steps: Improve the method to enhance the reaction efficiency. Explore alternative preparation methods for calcium carbonate to ensureplete conversion.
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Log Entry: September 6, 1657
Objective: Enhance the efficiency of calcium hydroxide production.
Today’s Experiment: Modified the setup to include a heated chamber to better react with calcium carbonate. The intended reactions were:
CaCO3?→CaO+CO2?
CaO+H2?O→Ca(OH)2?
Failure Analysis: The heating method used was rudimentary and failed to efficiently convert calcium carbonate into calcium oxide. Temperature control was poor, leading to iplete reactions and loss of carbon dioxide. Theck of proper containment resulted in inefficient conversion and low yield.
Next Steps: Investigate the use of a kiln for better temperature control and efficient conversion of calcium carbonate into calcium oxide. This should enhance the reaction and increase the yield of calcium hydroxide.