Calculate the energy required to produce 5.00 mol of Cl2O7 on the bases of the following balanced equation. 2Cl2(g) +7O2(g) +130kcal - - > 2 Cl2O7
5.00 kcal
65 kcal***
130 kcal
325 kcal
From the 'balanced equation', 2 moles Cl2O7 requires 130 kcals => normalizes to 1 mole Cl2O7 requires 65 kcals. From this 5 moles Cl2O7 then requires ... ??? You do the math.
To calculate the energy required to produce 5.00 mol of Cl2O7, we need to use the given balanced equation and the energy change associated with it.
The balanced equation is: 2 Cl2(g) + 7 O2(g) → 2 Cl2O7
The equation tells us that for every 2 moles of Cl2, 7 moles of O2, and 2 moles of Cl2O7, 130 kcal of energy is released.
Since the equation is balanced for 2 moles of Cl2O7, we can set up a proportion to find the energy required for 5.00 mol of Cl2O7:
2 moles Cl2O7 / 130 kcal = 5.00 moles Cl2O7 / x kcal
Cross-multiplying and solving for x, we get:
x = (5.00 mol Cl2O7 * 130 kcal) / 2 mol Cl2O7
x = 325 kcal
Therefore, the energy required to produce 5.00 mol of Cl2O7 is 325 kcal.