My teacher laid this much out for us but I don’t know how to get the products in each one.

Ammonia (NH3) boils at -33∘C; at this temperature it has a density of 0.81 g/cm3. The enthalpy of formation of NH3(g) is -46.2 k

Minchanka [31]

Answer:

-87098.82kJ

Explanation:

Hello,

This process could be attained into two steps due to the specified conditions at assuming that it is at -33°C at the beginning:

Δ $H=$ Δ $vapH+$ Δ $rH$

Thus:

Δ $vapH=5L*0.81\frac{kg}{L}*\frac{1000g}{1kg}*\frac{1molNH_3}{17gNH_3}*23.2\frac{kJ}{molNH_3}=5527.06kJ$

Once the ammonia is gaseous, the burning chemical reaction is:

$NH_3+\frac{3}{4} O_2-->\frac{1}{2}N_2+\frac{3}{2}H_2O$

So the enthalpy of reaction for the given amount of ammonia is:

Δ $rH=5L*0.81\frac{kg}{L}*\frac{1000g}{1kg}*\frac{1molNH_3}{17gNH_3}*(\frac{3}{2}*-290\frac{kJ}{mol}-(-46.2\frac{kJ}{mol}) ) =-92625.88kJ$

Finally, the total enthalpy is:

Δ $H=5527.06kJ-92625.88kJ=-87098.82kJ$

Best regards.

7 0

3 years ago

Write a balanced half-reaction for the reduction of permanganate ion (Mno) to manganese ion Mn?) in acidic aqueous solution. Be

Luden [163]

Explanation:

Permanganate is general name for the chemical compound which containes manganate (VII) ion. Permanganate(VII) ion is strong oxidizing agent as manganese is in +7 oxidation state and can be easily reduced and oxidize others.

The balanced half reaction for reduction of the permanganate ion, $MnO_4^-$ to manganese ion, $Mn^{2+}$ is shown below:

$MnO_4^-_{(aq)}+8H^+_{(aq)}+5e^-\rightarrow Mn^{2+}_{(aq)}+4H_2O_{(l)}$

6 0

3 years ago

What would happen to the boiling point of water at 8,000 m above sea level, where air pressure is lower?

mario62 [17]

it will get warm or spread out into the water or

5 0

3 years ago

Suppose there was a release of 1 mole of Alpha emission particle and 1 mole of Beta emission particles and both particles are ac

riadik2000 [5.3K]

Explanation:

translate the following word equation in the form of balance come alive with your number is aluminium + hydrochloric acid and Aluminium chloride + nitrogen

7 0

3 years ago

2.643 grams of potassium butanoate (KCH3(CH2)2CO2 ) is fully dissolved in 50.00 mL of water, which is carefully transferred to a

lara [203]

Answer:

The pH of the solution is 4.69

Explanation:

Given that,

Mass of potassium = 2.643 grams

Weight of water = 50.00 mL

Weight of HCl=100.00 ml

Mole = 0.120 M