Assuming the temperature and volume remain constant, changes to the pressure in the reaction vessel will directly

correspond to changes in the number of moles based on the ideal gas law $(PV=nRT).$

Suppose the reaction between nitrogen and hydrogen was run according to the amounts presented in Part A$,$ and the

temperature and volume were constant at values of $296K$ and $2\mathrm{.}00L,$ respectively. If the pressure was $11\mathrm{.}9$atm

prior to the reaction, what would be the expected pressure after the reaction was completed?

Express the pressure in atmospheres to three significant digits.

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pressure $=$

atm

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To solve this problem, use the equation derived from the ideal gas law in Hint $2$ to solve for pressure $(P).$

Values for temperature $(T),$ volume $(V),$ and the ideal gas constant $(R)$ have been given. In Part A$,$ you

determined the number of moles $(n)$ of gas particles present at the end of the reaction.

You may want to review Hint $1.$ How to apply the ideal gas law to determine pressure.