solution:
Let the heaviness of dihydrogen be 20 g.
Let the heaviness of dioxygen be 80 g.
No. of moles of dihydrogen (nH2),
![\[\begin{array}{*{35}{l}} ~ \\ =\text{ }20/2 \\ ~ \\ =\text{ }10\text{ }moles \\ ~ \\ No.\text{ }of\text{ }moles\text{ }of\text{ }dioxygen\text{ }\left( nO2 \right), \\ ~ \\ =\text{ }80/32 \\ ~ \\ =\text{ }2.5\text{ }moles \\ ~ \\ \end{array}\]](https://www.learnatnoon.com/s/wp-content/ql-cache/quicklatex.com-3016dcefcc96ffdf3368c87879955ca8_l3.png "Rendered by QuickLaTeX.com")
Given:
![\[ptotal\text{ }=\text{ }1\text{ }bar\]](https://www.learnatnoon.com/s/wp-content/ql-cache/quicklatex.com-6e161665a50388f20e87f3381f778f02_l3.png "Rendered by QuickLaTeX.com")
Hence, halfway tension of dihydrogen (pH2),
![\[=\text{ }0.8\text{ }bar\]](https://www.learnatnoon.com/s/wp-content/ql-cache/quicklatex.com-417369d642cda4e61315eff15e2dac59_l3.png "Rendered by QuickLaTeX.com")
Hence, the halfway tension of dihydrogen is 0.8 bar.
A combination of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Compute the halfway tension of dihydrogen.
A combination of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Compute the halfway tension of dihydrogen.