Answer:
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
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.
More on gas laws can be found here: https://brainly.com/question/1190311?referrer=searchResults
