The reaction below takes place in a closed, rigid vessel. The initial pressure of N2(g) is 1.0 atm, and that of O2(g) is 1.5 atm. No N2O4(g) is initially present. The experiment is carried out at a constant temperature. What is the total pressure in the container when the partial pressure of N2O4 reaches 0.75 atm?
N2+O2->N2O4
Please help and explain how you got the answer. I need help on got to get to the answer itself.
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The table compares the number of electrons in two unknown neutral atoms. comparison of electrons atom number of electrons a 9 d 11 use this information to determine the number of valence electrons in the atoms. which of the following correctly compares the stability of tthe table compares the number of electrons in two unknown neutral atoms. comparison of electrons atom number of electrons a 9 d 11 use this information to determine the number of valence electrons in the atoms. which of the following correctly compares the stability of the two atoms? both are unreactive. both are highly reactive. a is unreactive and d is reactive. a is reactive and d is unreactive.
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Phosphorous can form an ion called phosphide, which has the formula p3−. this ion can form an ion called phosphide, which has the formula p3−. this ion properties very similar to those of pforms when a phosphorus atom loses three protonsis called a cationcontains 18 electrons
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The reaction below takes place in a closed, rigid vessel. The initial pressure of N2(g) is 1.0 atm,...
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