Akira Yoshino Biography
Akira Yoshino is a Japanese chemist. Fellow of Asahi Kasei Corporation and professor of Meijo University. He is the inventor of lithium-ion battery (LIB) often used in cellular phones and notebook computers. He was awarded the Nobel Prize in Chemistry in 2019.
Akira Yoshino Age
Akira Yoshino was born on 30 January 1948. He is a Japanese chemist. Fellow of Asahi Kasei Corporation and professor of Meijo University. He is the inventor of lithium-ion battery (LIB) often used in cellular phones and notebook computers. He was awarded the Nobel Prize in Chemistry in 2019.
Akira Yoshino Height
Information concerning his height is still under research and will soon be updated immediately we come across details about his height.
Akira Yoshino Career
- 1972: Kawasaki Laboratory, Asahi Kasei Corp. / development of lithium-ion battery, etc.
- 1992: Manager, Product Development Group, Ion Battery Business Promotion Dept., Asahi Kasei Corp.
- 1994: Manager, Technical Development, A&T Battery Corp. (LIB manufacturer. Joint venture company of Asahi Kasei and Toshiba))
- 2003–present: Fellow, Asahi Kasei Corp. / researching next-generation themes
- 2005–present: General Manager, Yoshino Laboratory, Asahi Kasei Corp. / advanced battery research
Akira Yoshino Net Worth
Have you been wondering how rich is the Japanese chemist? According to our research, he has an estimated net worth of $8 Million.
Akira Yoshino Photo
Akira Yoshino Family
Information concerning his family is still under research and will soon be updated immediately we come across details concerning his height.
Akira Yoshino Nobel Prize
Three researchers were honored with a Nobel Prize in Chemistry this morning for their roles in the development of lithium-ion batteries, a technology that has made possible our mobile electronic world of cellular phones and electric cars. John Goodenough of the University of Texas, Austin, M. Stanley Whittingham of Binghamton University and Akira Yoshino of Meijo University share equally in the prize.
“Over two-thirds of the world’s population own a mobile device, be it a smartphone, a laptop or tablet, and nearly all powered by rechargeable lithium-ion batteries,” said Paul Coxon, a professor of materials science and metallurgy at the University of Cambridge, in an email. “They are the hidden workhorses of the mobile era, which came about thanks to fundamental research that began over 40 years ago.” Today’s prize honors the roles that Goodenough, Whittingham, and Yoshino each played in that transformational work.
When the researchers had started their work in the 1970s, the world was faced with an energy crisis and an environmental one, both of which had been building for decades. At the dawn of the electric era in the late 19th century, batteries were common fixtures of early automobiles and other devices. But they were heavy and inefficient, and research on improving them stagnated. Petroleum fuels quickly took over as the main source of energy used to power automobiles and other demanding systems.
But by the 1960s, the dangers of such heavy reliance on oil were becoming apparent. In the United States, oil shortages, coupled with smog-filled cities and other environmental dangers, made it clear that research was needed (and quickly) to find more sustainable ways of storing and using energy.
And so work on batteries made a comeback. In particular, scientists sought one that could take advantage of lithium, the lightest metal in the periodic table and material particularly predisposed to forming ions by giving up electrons. But “in order to use lithium in a battery, you really need to tame its reactivity,” said Olof Ramström, a professor of chemistry at the University of Massachusetts in Lowell and a member of the Nobel Prize committee, during the announcement today. “And that’s exactly what the work of the laureates has achieved.”
Batteries essentially store and release energy through a series of chemical reactions that occur at two electrodes, a positively charged cathode, and a negatively charged anode. Positive ions move from anode to cathode through an electrolyte between the two, which in turn prompts electrons to flow the other way through a circuit set up to power a connected device. This process is reversed to make the battery rechargeable.