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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Covalent bonds can be classified as nonpolar and polar covalent given the electronegativity difference between two atoms (ΔEN).
Nonpolar covalent bond electrons are shared equally between two atoms, polar covalent bond electrons are shared unequally, atoms have partial charges, ionic bond electrons are completely transferred to one atom, full charges present. Therefore, the greater the electronegativity difference, the greater the bond polarity. Let's determine the types of bonds present in the compounds and arrange the ones with polar covalent in order of increasing ΔEN. Phosphorus and fluorine are both nonmetals so the substance is covalent. Phosphorus has EN = 2.1 and fluorine has EN = 4.0. Given the large electronegativity difference, the P−F bonds in the substance can be classified as polar covalent bonds.
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There are 1.22 grams of He in the mixture. The mixture contains 0.304 moles of He, 0.250 moles of N2 and 0.250 moles of O2. Since the mixture of gases are at standard temperature and pressure, the total moles of the mixture equivalent to 18.0 L is 0.804 moles.
Further Explanation:
At standard temperature and pressure of 0°C and 1.00 atm, the molar volume of gas is 22.4 L.
From this, the total moles of the mixture can be derived using the solution below:
Therefore, the total moles of gases in an 18.0 L mixture at STP is:
By algebra, the moles of He may be solved using the given moles of the other two gases: 0.250 mol N2 and 0.250 mol O2.
0.304 moles of He is equal to 1.22 grams of He.
Learn More:
- Learn more about Boyle's Law brainly.com/question/12968820
- Learn more about Gay-Lussac's Law brainly.com/question/6534668
- Learn more about Ideal Gas Law brainly.com/question/12935899
Keywords: molar volume, STP, stoichiometry
Answer:
organic chemistry
Explanation:
There are many branches of chemistry. Some of them are physical chemistry, analytical chemistry, inorganic chemistry and organic chemistry.
A chemist is testing the quality of a wine produced by a vineyard. It means he will test the structure, properties, and preparation of wine. All these tests comes under organic chemistry.
Hence, the correct option is (d) "organic chemistry"
According to Henderson–Hasselbalch Equation,
pH = pKa + log [Lactate] / [Lactic Acid]
As,
Ka of Lactic Acid = 1.38 × 10⁻⁴
pKa = -log Ka
pKa = -log 1.38 × 10⁻⁴
pKa = 3.86
So,
pH = 3.86 + log [0.10] / [0.13]
pH = 4.74 + log 0.769
pH = 4.74 - 0.11
pH = 4.63