A chemist measures the energy change to be Delta H = 160 kJ during the following reaction. 2NH3(g) arrow N2(g) + 3H2(g) Suppose 44.2 grams of NH3 reacts. How much heat will be released or absorbed?

The given reaction is exothermic, meaning it releases heat. First, we need to determine the moles of NH3 that react. We can use the molar mass of NH3 (17.03 g/mol) to convert the given mass to moles: 44.2 g NH3 x (1 mol NH3/17.03 g NH3) = 2.59 mol NH3 From the balanced equation, we see that 2 moles of NH3 produces 3 moles of H2. Therefore, 2.59 moles of NH3 will produce: (2.59 mol NH3) x (3 mol H2/2 mol NH3) = 3.89 mol H2 Similarly, 2.59 moles of NH3 will produce 1.29 moles of N2: (2.59 mol NH3) x (1 mol N2/2 mol NH3) = 1.29 mol N2 Now we can use the given value of ?H to calculate the heat released: ?H = 160 kJ Heat released = ?H x (moles of NH3 reacted) Heat released = 160 kJ x 2.59 mol NH3 = 414.4 kJ Therefore, 44.2 grams of NH3 will react to release 414.4 kJ of heat.