In order to determine the velocity of gas molecules, it would not be unreasonable to measure the average velocity, vavg, of the gas molecules. However, the molecules of gas are constantly moving in completely random directions and this results in the average velocity being equal to 0 m/s.
The pressure of the gas <u>would increase.</u>
Explanation:
Using the ideal gas formulae we can evaluate this fact;
P₁V₁/T₁ = P₂V₂/T₂
We can assume that the volume is reduced by half (the T₁ and T₂ will cancel out because they remain constant);
P₁V₁ = P₂ * 0.5V₁
P₁V₁/0.5V₁ = P₂
P₁/0.5 = P₂
You can observe that the pressure will also increase – diving a number by a fraction or decimal number increases the resultant value. In this case, the pressure will increase by 2 fold
Answer:
The reaction will proceed to the left
Explanation:
<u>Step 1:</u> The balanced equation
CO(g) + H2O(g) ⇌ CO2(g) + H2(g)
<u>Step 2:</u> Data given
Kp = 2.7
Number of moles of CO = 0.13 mol
Number of moles of H2O = 0.56 mol
Number of moles of CO2 = 0.62 mole
Number of moles of H2 = 0.61 mol
Volume = 2.0L
Step 3: Calculate Q
Pco = 0.13 / 1.92 P
Ph2o = 0.56 / 1.92 P
Pco2 = 0.62/1.92 P
Ph2 =0.61 / 1.92 P
Q = [CO2][H2] / [CO][H2O] = 5.2
Q > Kp The reaction will proceed to the left
The reaction will proceed in the reverse direction in order to increase the concentrations of both CO and H2O and decrease that of CO2 and H2 until Q = K.