chem

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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asked by amber
  1. 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

    posted by DrBob222

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