Answer:
The entropy change for the vaporization of 18 grams of a hydrocarbon at its boiling point is 12.87 J/K.
Explanation:
Mass of hydrocarbon = 18 g
Molar mass of hydrocarbon = 114 g/mol
Moles of hydrocarbons =
The enthalpy of vaporization of hydrocarbon =
Heat required to heat 0.1579 moles of hydrocarbon = Q
Q = 4.263 kJ = 4,263 J ( 1 kJ = 1000 J)
Boiling point of hydrocarbon = T = 58.2°C = 58.2 + 273 K = 331.2 K
Entropy change for the vaporization of 18 g of a hydrocarbon:
The entropy change for the vaporization of 18 grams of a hydrocarbon at its boiling point is 12.87 J/K.
Consequences of oxygenation. Eventually, oxygen started to accumulate in the atmosphere, with two major consequences. Oxygen likely oxidized atmospheric methane (a strong greenhouse gas) to carbon dioxide (a weaker one) and water.
Answer:
Explanation:
Well At 0 °C and 1 atm pressure (STP conditions), ideal gases have a molar volume of 22.4 Liters. When the molar volumes of NH3 and CH4 are measured at STP, the molar volume of NH3 is 22.1 L and the molar volume of CH4 is 22.4 L. ... NH3 molecules take up more volume than CH4 molecules.
Answer:
You just have to take the periodic table of the elements, take the element that interests you. Then, you look at the formula of the element, at the top left you find the number of neutrons and protons and at the bottom left you find the number of protons. Then you just have to make the number from the top left minus the number from the bottom left.
Explanation:
If you are talking about the order of reaction in terms of the rate law you have to count all of the exponents in the rate law and that is the order of the reaction.
for example:
rate=k[A]⁰ would be a zero order reaction
rate=k[A] would be a first order reaction
rate=k[A]⁰[B] would also be a first order reaction
rate=k[A]² would be a second order reaction
rate=k[A][B] would also be a second order reaction
rate=K[A]³ would be a third order reaction
rate=k[A]²[B] would be a third order reaction as well
rate=k[A][B][C] would be a third order reaction as well
As you can in those examples to find the order of the reaction in terms of rate, all you need to do is add all of the exponents in the rate law formula.
I hope this helps. Let me know if you have any further questions or if you need anything to be clarified.