I'm not sure but it should be 7.31 times 2 times 3.14 or pi
7.31 x 2 x 3.14 = 45.9068
If you need to round to the nearest tenth it will be 45.9
If you need to round to the nearest hundredth it will be 45.91
Answer:
A
Explanation:
because number of particle = moles × 6.02 × 10^23
which gives the answer as an A
Answer:
H₂O.
Explanation:
- It is clear from the balanced equation:
<em>CH₄ + 2H₂O → CO₂ + 4H₂.</em>
that 1.0 mole of CH₄ reacts with 2.0 moles of H₂O to produce 1.0 mole of CO₂ and 4.0 moles of H₂.
- To determine the limiting reactant, we should calculate the no. of moles of (20 g) CH₄ and (15 g) H₂O using the relation:
<em>n = mass/molar mass</em>
<em></em>
no. of moles of CH₄ = mass/molar mass = (20 g)/(16 g/mol) = 1.25 mol.
no. of moles of H₂O = mass/molar mass = (15 g)/(18 g/mol) = 0.833 mol.
- <em>from the balanced reaction, 1.0 mole of CH₄ reacts with 2.0 moles of H₂O.</em>
So, from the calculated no. of moles: 0.4167 mole of CH₄ reacts completely with 0.833 mole of H₂O and the remaining of CH₄ will be in excess.
<u><em>So, the limiting reactant is H₂O.</em></u>
Answer:
32.00 g. Hope this helps! PLEASE GIVE ME BRAINLIEST!!!!! =)
Answer:
Explanation:
All three lighter boron trihalides, BX3 (X = F, Cl, Br), form stable adducts with common Lewis bases. Their relative Lewis acidities can be evaluated in terms of the relative exothermicities of the adduct-forming reaction. Such measurements have revealed the following sequence for the Lewis acidity: BF3 < BCl3 < BBr3 (in other words, BBr3 is the strongest Lewis acid).
This trend is commonly attributed to the degree of π-bonding in the planar boron trihalide that would be lost upon pyramidalization (the conversion of the trigonal planar geometry to a tetrahedral one) of the BX3 molecule, which follows this trend: BF3 > BCl3 > BBr3 (that is, BBr3 is the most easily pyramidalized). The criteria for evaluating the relative strength of π-bonding are not clear, however. One suggestion is that the F atom is small compared to the larger Cl and Br atoms, and the lone pair electron in the 2pzorbital of F is readily and easily donated, and overlaps with the empty 2pz orbital of boron. As a result, the [latex]\pi[/latex] donation of F is greater than that of Cl or Br. In an alternative explanation, the low Lewis acidity for BF3 is attributed to the relative weakness of the bond in the adducts F3B-L.
