Answer:
My name is Andreas Vesalius and I'm a 16th-century Flemish anatomist, physician, and author of one of the most influential books on human anatomy, De Humani Corporis Fabrica Libri Septem. I am often referred to as the founder of modern human anatomy. I was born in Brussels, December 31, 1514 which was then part of the Habsburg Netherlands. I was a Flemish doctor who was notable for my contribution to the science of anatomy of the human body. I was the first to perform public dissection on a human corpse, a practice that was unusual in the Middle Ages due to spiritual beliefs.
Explanation:
<u>Answer:</u> The correct IUPAC name of the alkane is 4-ethyl-3-methylheptane
<u>Explanation:</u>
The IUPAC nomenclature of alkanes are given as follows:
- Select the longest possible carbon chain.
- For the number of carbon atom, we add prefix as 'meth' for 1, 'eth' for 2, 'prop' for 3, 'but' for 4, 'pent' for 5, 'hex' for 6, 'sept' for 7, 'oct' for 8, 'nona' for 9 and 'deca' for 10.
- A suffix '-ane' is added at the end of the name.
- If two of more similar alkyl groups are present, then the words 'di', 'tri' 'tetra' and so on are used to specify the number of times these alkyl groups appear in the chain.
We are given:
An alkane having chemical name as 3-methyl-4-n-propylhexane. This will not be the correct name of the alkane because the longest possible carbon chain has 7 Carbon atoms, not 6 carbon atoms
The image of the given alkane is shown in the image below.
Hence, the correct IUPAC name of the alkane is 4-ethyl-3-methylheptane
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Answer:
1.195 g of Arsenic.
Explanation:
Equation of the reaction:
Ga(l) + As(s) → GaAs(s).
Calculating the limiting reagent by:
Number of moles of:
Gallium:
Molar mass of Gallium = 69.7 g/mol.
Mass = 4 g
Number of moles = mass/molar mass
= 4/69.7
= 0.0574 mol.
Arsenic:
Molar mass of Arsenic = 75 g/mol.
Mass = 5.5 g
Number of moles = mass/molar mass
= 5.5/75
= 0.0733 mol
Therefore, using stoichiometry since 1 mole of Gallium reacted with 1 mole of Arsenic. The limiting reagent is Gallium.
Excess reagent is Arsenic.
Number of moles excess = 0.0733 - 0.0574
= 0.0159 moles
Mass of the excess Arsenic left =
Molar Mass * number of moles
= 0.0159 * 75
= 1.195 g of Arsenic.