Respuesta :
Answer:
The change in total pressure is 0. There is no change in pressure.
Explanation:
Step 1: The balanced equation
CH4 + 2O2 → CO2 +2H20
Step 2: Data given
Temperature = 170 °C = 443 Kelvin
170 Torr of methane, CH4, and excess oxygen, O2
Step 3: Calcuate change of pressure
For 1 mole of CH4 consumed, we need 2 moles of O2. This means:
140 torr of CH4 means the pressure of O2 is at least 2*140 = 280 torr. Since it's excess it will be more so let's consider 280 + x torr
For 1 mole of CH4 consumed, we need 2 moles of O2, to consume 1 mole of CO2 and 2 moles of H2O. We can consider 140 torr of CO2 and 280 torr of H2O. Since we are at 170 °C, the water produced is vapor.
Of the excess O2, there will, after 280 torr is used, remain x torr of O2.
280 torr of O2 is used.
From the Ideal Gas Law: PV= nRT (all parameters are constant)
That means, P1 = P2
Thus, change in total pressure = 0 (no change)
