the temperature of a rigid (i. e constant volume) sealed container of gas increases from 100 C to 200 C the gas pressure increases by a factor of

The gas pressure would increase by a factor of 2.

At constant volume, the pressure of a gas increases with an increase in its temperature.

In this case, T1 = 100 and T2 = 200

            = 200/100

                  = 2

This means that the gas pressure would increase by a factor of 2 if the temperature were to be increased from 100 to 200 at constant volume.

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The pressure increases by a factor of 1.27

Explanation:

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

Initial temperature (T₁) = 100 °C

Final temperature (T₂) = 200 °C

Initial pressure (P₁) = P

Final pressure (P₂) =?

NOTE: The volume is constant.

Next, we shall convert celsius temperature to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 100 °C

Initial temperature (T₁) = 100 °C + 273

Initial temperature (T₁) = 373 K

Final temperature (T₂) = 200 °C

Final temperature (T₂) = 200 °C + 273

Final temperature (T₂) = 473 K

Next, we shall determine the final pressure of the gas. This can be obtained as follow:

Initial temperature (T₁) = 373 K

Final temperature (T₂) = 473 K

Initial pressure (P₁) = P

Final pressure (P₂) =?

P₁ / T₁ = P₂ / T₂

P / 373 = P₂ / 473

Cross multiply

373 × P₂ = P × 473

Divide both side by 373

P₂ = P × 473 / 373

P₂ = 1.27 × P

Finally, we shall determine the factor by which the pressure of the gas increase as follow:

Initial pressure (P₁) = P

Final pressure (P₂) = 1.27 × P

From the above, we can see that the pressure increased by a factor of 1.27

c is the answer because when something is left after something evaporates that shows the chemical change.