265.2 mmHg is the partial pressure of oxygen in 780 mmHg of total pressure.
Explanation:
The partial pressure of a gas is defined as the individual pressure of the gas in total mixture. In an ideal gas all the constituent gases have partial pressure some of which will give total pressure of the gas.
The partial pressure of a gas is calculated by
total pressure x mole fraction of the gas.
Mole fraction of the oxygen present is 0.34 as it is 34% of the total gas.
= 0.34 is the mole fraction
Total pressure is given as 780 mm Hg
The partial pressure can be calculated using the above formula:
Putting the values in equation:
780 x 0.34
= 265.2 mm Hg is the partial pressure of oxygen.
Answer:
Ag(s)
Explanation:
Metal atoms are held together by the metallic bond. The metallic bond consists of cations held together by a sea of mobile electrons.
Thus, the crystal of Ag(s) is composed of silver ions held together by a sea of mobile electrons. Electrostatic forces of attraction holds the crystal together.
<span>The correct answer should be two oxygen atoms. That's because it's properties are similar to carbon insofar that it can form four bonds, so if it forms bonds with 2 oxygen atoms then it will have all four bonds created since Oxygen forms double bonds. This would make SiO2 which is also known worldwide as silica.</span>
Answer:
Density = 4.191 gm/L
Explanation:
Given:
Molar mass = 93.89 g/mol
Volume(Missing) = 22.4 L (Approx)
Find:
Density at STP
Computation:
Density = Mass/Volume
Density = 93.89 / 22.4
Density = 4.191 gm/L
<u>Answer:</u> The equilibrium constant for 
equation is 
<u>Explanation:</u>
The given chemical equation follows:
The value of equilibrium constant for the above equation is 
Calculating the equilibrium constant for the given equation:
The value of equilibrium constant for the above equation will be:
Hence, the equilibrium constant for equation is
