In the following reaction, we start with $$2$$ moles of $$N2$$ and $$5$$ moles of $$H2$$ exerting a total pressure of $$7$$ atm at a given temperature in a closed vessel. When $$50$$% of $$N2$$ is converted into $$NH3N2+3H2$$⟶$$2NH3$$, partial pressure of $$NH3$$ is

Question

In the following reaction, we start with $$2$$ moles of $$N2$$ and $$5$$ moles of $$H2$$ exerting a total pressure of $$7$$ atm at a given temperature in a closed vessel. When $$50$$% of $$N2$$ is converted into $$NH3N2+3H2$$⟶$$2NH3$$, partial pressure of $$NH3$$ is

Infinity Learn · Accepted Answer

$$N2+3H2$$⟶$$2NH3$$ Taken                                  $$2$$        $$5$$           $$0$$   Reacted (50$$% of $$N2)        $$1$$        $$3$$       Left                                       $$1$$         $$2$$     Total moles of $$N2$$, $$H2$$ and $$NH3$$ $$=$$ $$5$$ mol initial mol $$=$$ $$7pressure$$ at start $$=$$ $$7$$ atmHence, pressure at equilibrium $$=$$ $$5$$ atm∴  Partial pressure of $$NH3=25$$×$$5=2atm$$

In the following reaction, we start with 2 moles of N2 and 5 moles of H2 exerting a total pressure of 7 atm at a given temperature in a closed vessel. When 50% of N2 is converted into NH3N2+3H2⟶2NH3, partial pressure of NH3 is

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