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Posted by on Tuesday, June 14, 2011 at 10:11pm.

According to the following thermochemical equation, what mass of H2O (in g) must form in order to produce 975 kJ of energy?

SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l), ΔH°rxn = -184 kJ

  • chemistry - , Tuesday, June 14, 2011 at 10:36pm

    184 kJ energy released in the formation of 2 moles(36 g) H2O. So
    36.0 g H2O x (975 kJ/184 kJ) = ??

  • chemistry - , Monday, November 21, 2011 at 3:45pm

    45

  • chemistry - , Friday, November 16, 2012 at 10:55pm

    what mass of Mg combines with 5.80 L of O2 measured at STP

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