How many moles of water (H₂O) molecules are in a 4.00 m3 container at a pressure 8.00 × 10⁵ N/m² and temperature 600°C? The ideal gas constant is R = 8.314 J/mol•K = 0.0821 L ∙ atm/mol ∙ K. A) 7.72 × 10²⁶ mol B) 641 mol C) 441 mol D) 3.86 × 10²⁶ mol E) 2.65 × 10²⁶ mol

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of water using the ideal gas law:

PV = nRT

where P = 8.00 × 10^15 N/m^2, V = 4.00 m^3, T = 600°C = 873 K, and R = 0.0821 L ∙ atm/mol ∙ K.

Solve for n:

n = PV/RT = (8.00 × 10^15 N/m^2)(4.00 m^3)/(0.0821 L∙atm/mol∙K)(873 K) = 441 mol

Therefore, there are 441 moles of water molecules in the 4.00 m^3 container. The correct answer is choice C.

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