Given: 8CO + 17H2 → C8H18 + 8H2O In this chemical reaction, how many grams of H2 will react completely with 6.50 moles of CO? Ex
2 answers:
Answer:- 27.6 grams of hydrogen are required.
Solution:- The given balanced equation is:
From balanced equation, there is 8:17 mol ratio between CO and means 17 moles of hydrogen are required to react completely with 8 moles of CO.
Let's calculate the number of moles of hydrogen required to react completely with 6.50 moles of CO and convert to grams on multiplying by molar mass of hydrogen as:
=
So, 27.6 grams of hydrogen are required to react completely with 6.50 moles of CO.
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Answer: 8.7 grams
Explanation:
According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number of particles.
To calculate the moles, we use the equation:
As oxygen is in excess, Aluminium is the limiting reagent and limits the formation of products.
According to stoichiometry:
4 moles of aluminium give = 2 moles of
Thus 0.17 moles of aluminium give=
Mass of
Thus the mass of is 8.7 grams
Answer:
Hybridization: sp
Electron geometry: linear
Molecular geometry: linear
Explanation:
H₃CCCH can also be written as its Lewis structure which is shown in the figure attached. The figure shows that the central carbon atom makes a single bond with CH₃ and a triple bond with CH. This means that the hybridization of the carbon is sp and both the electron and molecular geometry are linear with an 180° bond angle.
