Answer:
THE PARTIAL PRESSURE OF OXYGEN GAS IN THE CONTAINER IS 92.67kPa WHICH IS OPTION B.
Explanation:
To calculate the partial pressure of oxygen gas collected over water, we use
Ptotal = Poxygen + P water
It is worthy to note that when oxygen is collected over water, it is mixed with water vapor and the total pressure in the container will be the sum of the pressure exerted by the oxygen gas and that of the water vapor at that given temperature.
At 20 C, the vapor pressure of water as given in the question is 2.33 kPa.
Using the above formula,
Ptotal = Poxygen + P water
Substituting for Poxygen, we have;
Poxygen = Ptotal - P water vapor
P oxygen = 95 .00 kPa - 2.33 kPa
P oxygen = 92.67 kPa.
The partial pressure of oxygen gas in the container is hence, 92.67kPa.
Answer:
See explanation and image attached
Explanation:
The compound SF4 is sulphur tetraflouride. It has a zero formal charge and has a total of 34 valence electrons.
The central atom in the molecule is sulphur in an sp3d hybridization state hence the molecule has a trigonal bipyramidal electron geometry. Since it is a molecule of the sort AX4E; it gives a see-saw molecular shape.
The structure of the molecule is shown in the image attached to this answer.
Answer:
If Thomson's atomic theory was accurate, the positively charged particles would have gone through the foil.
Answer:
8×10^(-3) mol/L
Explanation:
The formula for finding the hydrogen ion concentration is...
[H⁺] = 10^-ph
[H⁺] = 10^(-2.1)
[H⁺] = 0.00794...mol/L = 8×10^(-3) mol/L
The answer is to 1 significant digit because the pH has one decimal place.
