Answer:
56.8cm³
Explanation:
Given parameters:
Measured volume = 54.5cm³
Percentage error = 4.25%
Unknown:
Actual volume of the cylinder = ?
Solution:
The percentage error shows the amount of error introduced into a measurement.
We need to find out this amount of error from the data given.
Error = Percentage error x measured volume
Error = x 54.5 = ±2.32cm³
Since the error introduced = 2.32cm³
Actual volume of cylinder = measured volume ± Error
Since the percentage error quoted as higher 4.25%;
Actual volume = 54.5cm³ + 2.32cm³ = 56.8cm³
Answer:
1) 1/√K
2) 1/K
3) √K
Explanation:
As general rules of operation of equilibrium constants:
For the reaction:
A + B ⇄ C + D; Equilibrium constant = K
C + D ⇄ A + B; K' = 1/K
2A + 2B ⇄ 2C + 2D; K'' = K²
Thus, as equilibrium constant of:
2CO2 + 4H2O ⇄ 2CH3OH + 3O2
Is K:
1) CH3OH + 3/2 O2 ⇄ CO2 + 2H2O
K' = 1 / K^(1/2) = 1/√K
2) 2CH3OH + 3O2 ⇄ 2CO2 + 4H2O
K' = 1/K
3) CO2 + 2H2O ⇄ CH3OH + 3/2 O2
K' = K^(1/2) = √K
Answer:
Pressure will increase by the direct ratio of the volume change. Therefore, since volume changes from 145 to 80, pressure will go up by the ratio change 145÷80 times the original pressure 125 kPa. Sure, you can use the more complicated gas law equation PV = nRT but we are only varying volume so the question boils down to the change in one simple variable.
Putting them together we have: 145÷80 x 125 = 226.5625 or just 226 kPa since the accuracy of the figures and the equation are not great.
Answer:
Explanation:
According to the Dalton's law of partial pressure, the total pressure of the gaseous mixture is equal to the sum of the pressure of the individual gases.
Partial pressure of carbon dioxide = 401 mmHg
Partial pressure of hydrogen gas = 224 mmHg
Total pressure,P = sum of the partial pressure of the gases = 401 + 224 mmHg = 625 mmHg
Also, the partial pressure of the gas is equal to the product of the mole fraction and total pressure.
So,
Similarly,
Answer:
FALSE
Explanation:
Energy is inversely proportional to wavelength.
∴ Waves with longer wavelengths have less energy than waves with shorter wavelengths.