According to the ideal gas law, partial pressure is inversely proportional to volume. It is also directly proportional to moles and temperature. At equilibrium in the following reaction at room temperature, the partial pressures of the gases are found to be PN2 = 0.094 atm, PH2 = 0.039 atm, and PNH3 = 0.003 atm.
<h3>Equilibrium partial pressures</h3>
The initial partial pressures of CO and water are 4.0 bar and 4.0 bar respectively.
The equilibrium partial pressures (in the bar) of CO, H2O, CO2, and H2 are 4−p,4−p, and respectively.
Let p bar be the equilibrium partial pressure of hydrogen.
The expression for the equilibrium constant is
Kp=PCOPH2OPCO2PH2=(4−p)(4−p)p×p=0.1
p=1.264−0.316p
p=0.96 bar.
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Ionization of H2CO3
<span>Step-1: </span>
<span>H2CO3 (aq) + H2O (l) <----> HCO3- (aq) + H3O+ (aq) </span>
<span>Step-2: </span>
<span>HCO3- (aq) + H2O (l) <----> CO32- (aq) + H3O+ (aq) </span>
<span>Ionization of H3BO3 </span>
<span>Step 1 is </span>
<span>H3BO3(aq) + H2O(l) <=> H2BO3-(aq) + H3O+(aq) </span>
<span>Step-2: </span>
<span>H2BO3-(aq) + H2O(l) <=> HBO3^-2(aq) + H3O+(aq) </span>
<span>Step 3 is</span>
<span>HBO3^-2(aq) + H2O(l) <=> BO3^-3(aq) + H3O+(aq)
credits go to Mary Nancy :)</span>
Answer:
has two double C-C bonds
Explanation:
A saturated compound is a compound having the full complement of hydrogen atoms for every carbon atom while an unsaturated compound does not contain the full complement of hydrogen atoms for every atom of carbon.
If we look at C3H4, the only possible structure of the compound is H2C=C=CH2. We can see from this arrangement that the compound contains a cumulative double bond. This is the specific structure that fits into one of the descriptions in the options, the compound contains two double bonds.
Answer:
1.39
Explanation:
1060 mm / 760 mm/atm = 1.39 atm
The answer to this would be b ,