The form of nitrogen monoxide, NO fromN2(g)and O2(g), requires 21.6 kcal of heat

Question

   The form of nitrogen monoxide, NO fromN2(g)and O2(g), requires 21.6 kcal of heat. N2(g) + O2(g) -------> 2NO(g)     H = 21.6kcal a. How many kcal are required to form 3.00 g NO? b. What is the complete equation (including heat) for thedecomposition of NO? c. How many kcal are released when 5.00 g NO decompses to N2and O2?    The form of nitrogen monoxide, NO fromN2(g)and O2(g), requires 21.6 kcal of heat. N2(g) + O2(g) -------> 2NO(g)     H = 21.6kcal a. How many kcal are required to form 3.00 g NO? b. What is the complete equation (including heat) for thedecomposition of NO? c. How many kcal are released when 5.00 g NO decompses to N2and O2?

Explanation / Answer

1) Based on this formula it states that we need 21.6 kcal for2 moles of NO to form. This means that we need 10.8 kcal for 1mole. To form 3 grams, first we need to figure out how many moles wehave 3 grmas/30 grams/mol = .1 moles NO Multiply .1 moles X 10.8 kcal/mol = We need 1.08kcal heat to form 3 grams NO 2) The decompoisiton reaction is the exact reverse of theequation given so it would be 2NO (g) -------> N2(g) + O2(g) + 21.6 kcalheat. Since this is the reverse of the reaction 21.6kcal of heat is released and not used up. 3) Apply the same formula as in question 1: 5 grams = .166moles NO .166 moles NO X -10.8 kcal heat release/mol = 1.8 kcalheat released Good Luck Good Luck

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