On a topographic map, the contour lines follow a certain elevation across the terrain. So here's what each of the things you mention would mean: If the lines are far apart, that means that there is little or no slope in that area of the map
Rank the gas molecules CO2, C2H6, H2O, He, H2 in terms of increasing rate of effusion. 1. CO2, C2H6, H2O, He, H2 2. CO2, C2H6, H
Kipish [7]
Ranking the gas molecules in terms of increasing rate of effusion is given as CO2, C2H6, H2O, He, H2
<u>Explanation:</u>
- The rate of effusion a gas is reciprocal to the square root of its molecular weight. The rate of effusion is to be arranged in the increasing rate of effusion.
- Arranging in terms of expanding rate of effusion, that is from heaviest to lightest molecule, (for example from smallest to highest effusion rate). The rate of effusion is higher for lighter molecule and also it effuses slowly.
Molar mass of CO2 = 44.01 g/mol
Molar mass of C2H6 = 30.07 g/mol
Molar mass of H2O = 18.01 g/mol
Molar mass of He = 4 g/mol
Molar mass of H2 = 2.01 g/mol
- When the molecule has a high molecular weight, it slows the rate of effusion. Hence the gas molecules are arranged as CO2, C2H6, H2O, He, H2
Answer
× 10²³ molecules are in 41.8 g of sulfuric acid
Explanation
The first step is to convert 41.8 g of sulfuric acid to moles by dividing the mass of sulfuric acid by its molar mass.
Molar mass of sulfuric acid, H₂SO₄ = 98.079 g/mol
Finally, convert the moles of sulfuric acid to molecules using Avogadro's number.
Conversion factor: 1 mole of any substance = 6.022 × 10²³ molecules.
Therefore, 0.426187053 moles of sulfuric acid is equal
Thus, 2.57 × 10²³ molecules are in 41.8 g of sulfuric acid.
The data for the heat of fusion for the isopropyl alcohol is 3.301 kJ/mol. This data was taken from Parks and Kelly (1928). After acquiring this data, we can now calculate for the amount of heat:
(3.301 kJ/mol) x (1. 37 mol) = 4.52 kJ
Thus, the amount of heat required to completely melth 1.37 mol of solid isopropyl alcohol at its melting point (184 K) is 4.52 kJ.