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Calculate the total pressure in a mixture of `8 g` of oxygen and `4 g` hydrogen confined in a vessel of `1 dm^(3)` at `27^(@)C`. `(R = 0.083 "bar" dm^(3) K^(-1) mol^(-1))` |
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Answer» Correct Answer - 65.025 bar Given, mass of dioxygen `(O_(2))` = 8 g Thus, numbe of moles of `O_(2)=8/32=0.25`mole Thus number of moles of `H_(2)=4/2=2` mole Therefore, total number of moles in the mixture =0.25+2=2.25 mole Given, V= 1 `dm^(3)` n= 2.25 mol R= 0.083 bar `dm^(3)K^(-1)mol^(-1)` T= `27^(@)C`=300K Total pressure (p) can be calculate as : pV= nRT `rArr=(nRT)/V` `=(225xx0.083xx300)/1` =56.025 bar Hence, the total pressure of the mixture is 56.025 bar. |
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