Question

assuming stp and a stoichiometric amount of nh3 and no in an expandable container originally at 15 L, what is the final volume if the reaction goes to completion? 4NH3 (g) + 6NO (g) —> 5N2 (g) + 6H2O (g)

Answer 1

16.5 L

Step-by-step explanation:

We are given the following factors (they are all essential):

• 4 moles NH3 gas (15 L initially)
• 6 moles NO gas
• Container volume = 15 L initially at STP

Given reaction:

4NH3 (g) + 6NO (g) -> 5N2 (g) + 6H2O (g)

Using the mole ratios from the balanced chemical equation:

For every 4 moles NH3, there will be 6 moles NO and they will react to produce:

• 5 moles N2
• 6 moles H2O

Initial moles of gas:

• 4 moles NH3
• 6 moles NO
• Total = 10 moles

Final moles of gas:

• 5 moles N2
• 6 moles H2O
• Total = 11 moles

By Avogadro's law, volume is directly proportional to moles of gas at constant temperature and pressure.

Since we have 11 moles of gas after the reaction compared to 10 moles initially, the final volume will be:

(11 moles gas)(15 L initial)/(10 moles initial)

= 16.5 L

So in summary, the final volume of the gas mixture after the reaction goes to completion will be 16.5 L, assuming a constant temperature and pressure within the expandable container.

The general approach is to calculate the mole ratios and number of moles of gases before and after the reaction, then use proportionality to determine how the volume will change accordingly.