2 N2 (g) + O2 (g) ---> 2 N2O (g) H= +163.2 kj/mol How much heat is required to produce 25.0 g of N2O by this reaction? Show all calculations.

46.3 kJ

Explanation:

Step 1: Write the thermochemical equation

2 N₂(g) + O₂(g) ⇒ 2 N₂O(g)  ΔH= +163.2 kJ/mol

Step 2: Calculate the moles corresponding to 25.0 g of N₂O

The molar mass of N₂O is 44.01 g/mol.

25.0 g × (1 mol/44.01 g) = 0.568 mol

Step 3: Calculate the heat released when 0.568 moles of N₂O are produced

According to the thermochemical equation, 163.2 kJ are required per 2 moles of N₂O.

0.568 mol × (163.2 kJ/2 mol) = 46.3 kJ

you did not give any options thus this is the best answer i can give to you with this little information you have given

> they are both natural and not man made

> they can be tracked and predicted by the right tools

-love shrooms

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.