Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ___ NH3(g) + ___ O2(g) → ___ NO(g) + ___ H2O(l)

→

Volume of NO = 11.46 lit

Explanation:

From the above written equation we can easily understood that here acts as an limiting reagent.

4 mol of can produce 4 mol of

Molecular weight of = 17 g/mol

So, 8 g of means = = 0.470 mol

So, 0.470 mol of will produce 0.470 mol of NO

Molecular weight of NO = 30 g/mol

So, 0470 mol of NO means (30 × 0.470 ) = 14.1 g

we know that, Density =

 Volume of NO = = 11.46 lit  

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

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