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P4(s)+Cl2(g)–PCl5(g) balance the chemical reaction equation?
Enter the coefficients in order, separated by commas (e.g., 1,2,3).
Consider a situation in which 186g of P4 are exposed to 208g of O2.
What is the maximum amount of P2O5 that can theoretically be made from 186g of P4 and excess oxygen?
What is the maximum amount of P2O5 that can theoretically be made from 208g of O2 and excess Phosphorus?
Thank you very much for your help. This chapter is hard!
Given the following reactions P 4 s 10 Cl 2 g 4 PCl… | Course Hero – This preview shows page 5 – 8 out of 8 pages. 15. Given the following reactions P4(s) + 10 Cl2(g) → 4 PCl5(s) ΔrH = -1774.0 kJ/mol PCl3(l) + Cl2(g) ___ 18. What is the correct standard thermochemical expression for the formation of H2O? a. H2(g) + ½ O2(g) → H2O(l) ΔH° = -285.8 kJ b. H2(g) + ½ O2…Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=? by making use of the following information: P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019 PCl5(g)⇌PCl3(g)+Cl2(g)We'll balance the most complex compound first: #PCl_5#. The easiest way to do this is to balance the #P# since the ratio of #P:PCl_5# in #PCl_5# is #1:1#. By making the coefficient of #Cl_2# in the reactants side 10, we end up with 20 #Cl# atoms on each side. Overall, we now have 4 #P# and 20…
Chapter 14- Chemical Equilibrium Flashcards | Quizlet – P4(s) + 6 Cl2(g)–> 4 PCl3(l) ΔH°f = ? The percentage yield for the reaction PCL3+Cl2–>PCL5 is 83.2%. What mass of PCL5 is expected from the reaction of 73.7g of PCL3 with excess chlorine?4PCl₅(g)⇌P₄(s)+10Cl₂(g) Kgoal = ?# P_4 (s) + 10Cl_2 (g) rarr 4PCI_5 (s) #. Jag finner multiplikationen lite lättare att hantera om du använder den tidigare ekvationen. Och sålunda, med den givna stökiometrin med avseende på fosfor, kan vi göra # 0,177 * molxx4 = 0,710 * mol # med avseende på # PCl_5 #.
How do you balance P_4(s) + Cl_2(g) -> PCl_5(g)? | Socratic – P4 + 6Cl2 ==> 4PCl3 balanced equation. (2) convert 12.3 g P4 to moles and calculate theoretical yield of PCl3 in moles (3) covert moles PCl3 to grams PCl3 theoretically formed: 0.3972 moles PCl3 x 137.3 g/mol = 54.5g PCl3 = theoretical yield.Calculate the number of moles of PCl5 that can be produced from 53.0 g of Cl2 (and excess P4). Then, compare the two values. The reactant that produces the smaller amount of product is the limiting reactant.Part B How many moles of PCl5 can be produced from 26.0 g of P4 (and excess Cl2)? Express your answer to three significant figures and include the appropriate units. 0.333 mole….answer to C. Part D What mass of PCl5 will be produced from the given masses of both reactants?
Oxidizing Agents and Reducing Agents – .
C2H2 Lewis Structure Tutorial – How to Draw the Lewis Structure for Ethyne or Acetylene – OK, let's try the Lewis structure for C2H2:
We have it right here. You can see the Hydrogens on the outside, two Carbons
in the middle. What's all this? We'll see in a minute. So, first thing we need to do,
count those valence electrons for C2H2. We have a periodic table. Carbon is in group
14, or 4A, so it has 4 valence electrons. Carbon has 4. Over here, Hydrogen, in group
1A or 1, that has 1 valence electron, but since I have two Carbons, let's multiply that
by 2; and I have two Hydrogens, multiply that by 2, so that equals 8, that equals 2; I add
them up, I have 10 valence electrons to work with in this Lewis structure here. So with
10 valence electrons, let's see where we go next. Put the least electronegative atom at
the center. But Hydrogen always goes on the outside. So here it's pretty easy. We've got
Carbon, Carbon, and Hydrogen has to go on the outside. All right. Assign two electrons
to each bond. Let's put two here, let's put two here, two here, so we've used 2, 4, 6.
So we've only got 4 valence electrons left to work with. So we've assigned two electrons
to each bond. Now we need to complete the octets on the outside atoms. In this case,
Hydrogen right here is already full. It's the exception. It only needs 2 valence electrons
to be full, to have a full outer shell or octet. Everything else needs 8, but Hydrogen
needs 2. So we've got 4 valence electrons. Let's put the remaining electron pairs on
the central atom, or in this case, atoms. So I need to get 8 around each one. So there's
2, 2. So i've used all my valence electrons, Hydrogens are fine. Two, 4, 6, 8, that Carbon's
fine. But this Carbon right here only has 2, 4 valence electrons. So its octet is not
complete. It's not a stable molecule that way. So we need to figure out something, somehow
to get 8 valence electrons around this Carbon, this Carbon, and keep the Hydrogens full.
If the central atom doesn't have an octet, what we'll need to do is pull some electrons
in and share them, to make each atom have more electrons. So let's take these two right
here, and we'll put them right here. So now Hydrogens are fine. This Carbon has 2, 4,
6, 8, because it's sharing, right, and this Carbon has 2, 4, 6. Not quite there yet. Let's
move another pair in. Let's take those, put them right here. I'm going to make these a
little darker. And now Hydrogens are fine. This Carbon has 2, 4, 6, 8; it has an octet.
And this Carbon has 2, 4, 6, 8; it has an octet. And if we count them all up, we have
2, 4, 6, 8, 10 valence electrons, which is what we had to start with, and we've written
the Lewis structure for C2H2. We can clean it up a little bit to make it easier to see
here. And you notice all those valence electrons being shared in the center. We could write
this as, using these lines. Each line represents a pair of electrons. That's one way to do
it. And if you come back to our structure, now you can see these are the single bonds
right here. And this triple bond, 1, 2, 3, in the center, holds the two Carbons together–bonds
those together. That's the Lewis structure for C2H2, ethyne. .
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