A sample of nitrous oxide has a volume of 120 L at 1.500 mm Hg and = 10°C. Calculate its pressure when its volume is compressed to 50 L and its temperature increased to
34°C

3.91 mmHg

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 120 L

Initial pressure (P₁) = 1.5 mmHg

Initial temperature (T₁) = 10 °C

Final volume (V₂) = 50 L

Final temperature (T₂) = 34 °C

Final pressure (P₂) =?

Next, we shall convert 10 °C and 34 °C to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 10 °C

Initial temperature (T₁) = 10 °C + 273

Initial temperature (T₁) = 283 K

Final temperature (T₂) = 34 °C

Final temperature (T₂) = 34 °C + 273

Final temperature (T₂) = 307 K

Finally, we shall determine final pressure of the gas as follow:

Initial volume (V₁) = 120 L

Initial pressure (P₁) = 1.5 mmHg

Initial temperature (T₁) = 283 K

Final volume (V₂) = 50 L

Final temperature (T₂) = 307 K

Final pressure (P₂) =?

P₁V₁/T₁ = P₂V₂/T₂

1.5 × 120/283 = P₂ × 50 / 307

Cross multiply

P₂ × 50 × 283 = 1.5 × 120 × 307

P₂ × 14150 = 55260

Divide both side by 14150

P₂ = 55260 / 14150

P₂ = 3.91 mmHg

Thus, the new pressure of the gas is 3.91 mmHg

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explanation:

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.