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How much B5H9 must be burned to produce 4500 kcal of energy by following equation 2B5H9+12O2=9H2O+5B2O3 delta H=-4188 kcal/mole
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An analysis of an oxide of nitrogen with a molecular weight of92.02 amu gave 69.57% oxygen and 30.43 % nitrogen. What is the empirical formula of the compound?
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