2.11 moles of C₃H₈ are allowed to burn in the presence of excess O₂ to form CO₂ and H₂O.

C₃H₈(g) + 5 O₂(g) $\rightarrow$ 3 CO₂(g) + 4 H₂O(g)
The carbon dioxide is isolated from all other gases and stored in a 1.25 L container at 0.00°C. What is the pressure in this container if the gas obeys the ideal gas equation?

Question

2.11 moles of C₃H₈ are allowed to burn in the presence of excess O₂ to form CO₂ and H₂O.

C₃H₈(g) + 5 O₂(g)

\rightarrow

3 CO₂(g) + 4 H₂O(g)
The carbon dioxide is isolated from all other gases and stored in a 1.25 L container at 0.00°C. What is the pressure in this container if the gas obeys the ideal gas equation?

Quizplus · Accepted Answer

The ideal gas equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. We can rearrange this equation to solve for P: P = nRT/V.We are given that n = 2.11 moles, V = 1.25 L, R = 0.0821 L*atm/(mol*K), and T = 0.00°C = 273.15 K. Plugging these values into the equation, we get:P = (2.11 moles * 0.0821 L*atm/(mol*K) * 273.15 K) / 1.25 L = 113 atmTherefore, the pressure in the container is 113 atm.

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