C4H8N8O8(s) → 3 CO2(g) + C(s) + 2 H2O(g) + 2 H2(g) + 4 N2(g)Consider the above balanced equation. If the decomposition of C4H8N8O8(s) produces a total pressure of 3.7 atm, what is the partial pressure of elemental gas?A.0.67 atmB.1.3 atmC.1.8 atmD.2.0 atm
Question
C4H8N8O8(s) → 3 CO2(g) + C(s) + 2 H2O(g) + 2 H2(g) + 4 N2(g)Consider the above balanced equation. If the decomposition of C4H8N8O8(s) produces a total pressure of 3.7 atm, what is the partial pressure of elemental gas?A.0.67 atmB.1.3 atmC.1.8 atmD.2.0 atm
Solution
The balanced equation shows that for every 1 mole of C4H8N8O8 decomposed, 1 mole of carbon (C) is produced.
The total pressure produced by the decomposition is the sum of the partial pressures of all the gases produced.
Given that the total pressure is 3.7 atm, and that the gases produced are CO2, C, H2O, H2, and N2, we can calculate the partial pressure of each gas by dividing the total pressure by the number of moles of gas produced.
From the balanced equation, we can see that the number of moles of gas produced is 3 (from CO2) + 1 (from C) + 2 (from H2O) + 2 (from H2) + 4 (from N2) = 12 moles.
Therefore, the partial pressure of each gas is the total pressure divided by the number of moles of gas, which is 3.7 atm / 12 moles = 0.308 atm per mole of gas.
Since the balanced equation shows that 1 mole of C is produced, the partial pressure of C is 0.308 atm.
However, this option is not available in the choices given. It seems there might be a mistake in the question or the choices provided.
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