Question
If boron hydride, B4H10, is treated with pure oxygen, it burns to give B2O3 and H2O.
2 B4H10(s) + 11 O2(g) 4 B2O3(s) + 10 H2O(g)
If a 0.050-g sample of the boron hydride burns completely in O2, what will be the pressure of the gaseous water in a 4.25-L flask at 30. °C?
2 B4H10(s) + 11 O2(g) 4 B2O3(s) + 10 H2O(g)
If a 0.050-g sample of the boron hydride burns completely in O2, what will be the pressure of the gaseous water in a 4.25-L flask at 30. °C?