Suppose 0.500 moles of tungsten hexafluoride gas reacts with 1.500 moles of hydrogen gas with a total pressure of 2.21 atm at 400.00 $\circ$ C in a 50.0 L deposition chamber to form tungsten metal and hydrogen fluoride gas,which are then cooled to 0.00 $\circ$ C.What is the final pressure? WF₆(g)+ 3 H₂(g)$\to$ W(s)+ 6 HF(g)

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The reaction consumes 0.500 moles of WF6 and 1.500 moles of H2, producing 3.00 moles of HF. Using the ideal gas law and considering the temperature change, the final pressure is calculated to be 1.35 atm.

Suppose 0500 Moles of Tungsten Hexafluoride Gas Reacts with 1 ∘\circ∘

Suppose 0500 Moles of Tungsten Hexafluoride Gas Reacts with 1 $\circ$