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 4.7 L life belt with hydrogen gas at 1.04 atm and 22.4°C?
how do i even start this problem?
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Use PV = nRT to calculate moles H2 gas needed. Then put the H2 in the equation given and use stoichiometry to convert moles H2 to moles LiH, then to grams LiH
1 answer