Explanation:
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Answer:
I think that the statement is relative to speed because it is saying km per second.
Benzene reacts with O₂ to produce CO₂ and H₂O, i.e.
C₆H₆ + 7.5 O₂ → 6 CO₂ + 3 H₂O
According to equation,
78.11 g (1 mole) C₆H₆ reacts to produce = 264 g (6 moles) of CO₂
Hence,
7.80 g C₆H₆ when reacted will produce = X g of CO₂
Solving for X,
X = (7.80 g × 264 g) ÷ 78.11 g
X = 26.36 g of CO₂
Theoretical Yield:
26.36 g of CO₂ produced is theoretical yield which shows 100% reaction between benzene and oxygen.
Actual Yield:
According to statement the actual amount of CO₂ produced is 3.0 g of CO₂.
%age Yield:
%age Yield = (Actual Yield ÷ Theoretical Yield) × 100
Putting Values,
%age Yield = (3.00 g ÷ 26.36 g) × 100
%age Yield = 11.38 %
Answer:
Nitrogen reacts with oxygen to form a number of nitrogen oxides. It exhibits different oxidation states in its oxides, ranging from +1 to +5. Oxides of nitrogen having nitrogen in the higher oxidation state are more acidic than that in lower oxidation state. Nitrogen oxides are critical components of photochemical smog. They produce the yellowish-brown colour of the smog. In poorly ventilated situations, indoor domestic appliances such as gas stoves and gas or wood heaters can be significant sources of nitrogen oxides.
Following are the harmful effects caused by the oxides of nitrogen
Nitrogen oxides causes irritation in mucous membrane.
Large concentrations of Nitrogen oxide causes lungs problems in humans
It causes injuries to vegetation by damaging leaves.
Nitrogen oxide oxidizes Hydrocarbons in the presence of sunlight, which causes eye irritation, asthama attacks, nasal and throat infections.
NO: sharp, sweet-smelling, colourless gas. Melting point: -163.6°C. Boiling point: -151.8°C. Relative Density: 1.04 (air = 1) NO2: reddish-brown gas with irritating odour
