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Lithium hydride reacts with water as follows...?
Lithium hydride reacts with water as follows.
LiH(s) + H2O(l) LiOH(aq) + H2(g)
During World War II, U.S. pilots carried LiH tablets. In the event of a crash landing at sea, the LiH would react with the seawater and fill their life belts and lifeboats with hydrogen gas. How many grams of LiH are needed to fill a 4.1 L life belt at 0.97 atm and 10°C?
I am so confused? Any help is appreciated.
1 Answer
- Dr OChemLv 61 decade agoFavorite Answer
This is just a mole mole calculation. Convert 4.1 L of gas to STP from 0.97 atm and 10°C. Calculate the number of moles from that.
Now, since it takes two moles of LiH to make one mole H2. Take your moles of H2 you calculated above and multiple x 2. That is the number of moles LiH. Multiply the number of moles x g/mole of LiH. Voila, the answer.
