O₂ required = 1/2 x 7.8 = 3.9 moles
Answer:
In writing the electron configuration for nitrogen the first two electrons will go in the 1s orbital. Since 1s can only hold two electrons the next 2 electrons for N goes in the 2s orbital. The remaining three electrons will go in the 2p orbital. Therefore the N electron configuration will be 1s22s22p3.
Explanation:
hope you get it right:)
This is where something called Graham's Law applies. Grahams law says that the rate of effusion is inversely proportional to the square root of the molar mass of a gas. What that means is that the less the molar mass of a gas is, the less quickly the gas effuses (effusion being the rate at which a gas can travel through a small hole). A great way to think about this is that effusion is thought about as though the gas is traveling through a small hole, so smaller particles would be able to go through it with greater ease than would a large particle. I don't know what particular sentences the question asks for are, but the answer should be that gas A (molar mass 4) has the greatest effusion rate, gas B (molar mass 16) has the second fastest effusion rate, and gas C (molar mass 32) has the slowest effusion rate.
Answer: 170.9 g
Explanation:
1) Balanced chemical equation:
Fe₂O₃(s) + 6 H₂C₂O₄ (aq) → 2Fe(C₂O₄)₃³⁻ + 3H₂O + 6H⁺(aq)
2) mole ratio:
1mol Fe₂O₃ : 6 mol H₂C₂O₄
3) number of moles of H₂C₂O₄ in the solution
M = n / V ⇒ n = MV = 0.800M × 0.800 liter = 6.40 moles
4) Porportionality
1mol Fe₂O₃ / 6 mol H₂C₂O₄ = x / 6.40 mol H₂C₂O₄
⇒ x = 1.07 mol Fe₂O₃
5) Convert 1.07 mol Fe₂O₃ to grams.
molar mass Fe₂O₃ = 159.69 g/mol
mass in grams = molaer mass × number of moles
mass in grams = 159.69 g/mol × 1.07 mol = 170.9 g
Considering the ideal gas law, the pressure of the gas sample is 122.18 atm.
<h3>What is an ideal gas</h3>
An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.
<h3>Definition of ideal gas law</h3>
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of gases:
P×V = n×R×T
<h3>Pressure of the gas sample</h3>
In this case, you know:
- P= ?
- V= 500 mL= 0.5 L
- n= 2.50 moles
- R= 0.082
- T= 25 °C= 298 K
Replacing in the ideal gas law:
P×0.5 L = 2.50 moles ×0.082 ×298 K
Solving:
P= (2.50 moles ×0.082 ×298 K)÷ 0.5 L
<u><em>P= 122.18 atm</em></u>
Finally, the pressure of the gas sample is 122.18 atm.
Learn more about the ideal gas law:
brainly.com/question/4147359
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