Answer to Question #327830 in General Chemistry for Jas

Question

A 4.00 L rigid vessel (see figure below) holds 2.00 L of pure water. The remaining volume holds N2 at 45.0°C. At this stage the pressure gauge on the vessel reads 85.0 kPa. You then load 13.2 g of Be(NO3)2(s) and 15.4 g of N2H5Cl(s) to the container. The salts dissociate completely and a reaction occurs producing both NO(g) and more N2(g). After the reaction has completed, the temperature increased by 5.00°C, with no change in the liquid volume.

Assume that:

o No gas escaped or entered the vessel during the loading of the reagents.

o The liquid phase is free of any gaseous species.

o The ideal gas law applies.

o The reaction is irreversible with a yield of 88.0%.

i. Show that the balanced reaction in alkaline (basic) medium is given by:

4𝑁𝑂3 − (𝑎q) + 3𝑁2𝐻5 + (𝑎q) → 4𝑁𝑂(𝑔) + 3𝑁2(𝑔) + 7𝐻2𝑂(l) + 𝑂𝐻(𝑎q) −

(Show all balancing steps clearly)

ii. Calculate the number of moles of N2(g) and NO(g) after the reaction.

iii. Calculate the partial pressure of N2(g) and NO(g) in kPa after the reaction

Answer 1

I'm sorry, I don't have time to do this task