Consider the reaction shown:
N₂ + O₂ → 2 NO ΔH = 43.2 kcal
When 50.0 g of N₂ react,________ kcal will be ________.

Question

Consider the reaction shown: N₂ + O₂ → 2 NO ΔH = 43.2 kcal When 50.0 g of N₂ react,________ kcal will be ________.

Quizplus · Accepted Answer

To solve this, first, we need to calculate the molar mass of $N_2O$ (which is the product, but we'll use it to find out how many moles of $N_2$ react, assuming the reaction goes to completion and all $N_2$ is used). The molar mass of $N_2O$ is approximately 44.01 g/mol (28.01 for $N_2$ + 16.00 for $O$). Given that 50.0 g of $N_2$ react, we find the moles of $N_2$ by dividing the mass by its molar mass (approximately 28.01 g/mol), which gives us about 1.785 moles of $N_2$. Since the reaction shows a 1:1 mole ratio between $N_2$ and $N_2O$, we would produce the same amount of moles of $N_2O$.The given $\Delta H$ is 43.2 kcal for the production of 2 moles of $NO$, but since we're dealing with $N_2O$ in the question, there seems to be a misunderstanding in the chemical equation provided. Assuming the question meant $2NO$ as the product and considering the stoichiometry of the reaction, the energy change would be directly proportional to the amount of $N_2$ reacted.Given that 43.2 kcal is for the reaction as written, for 1 mole of $N_2$ reacting, we would have 43.2 kcal. For 1.785 moles, the energy change ($\Delta H$) would be $43.2 \, \text{kcal/mole} \times 1.785 \, \text{moles} = 77.1 \, \text{kcal}$.Since the reaction is endothermic ($\Delta H > 0$), this energy is consumed.

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