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Anestetic [448]
3 years ago
4

Which is the Lewis structure for H3PO4?

Chemistry
2 answers:
Vladimir [108]3 years ago
8 0
<span>There are a total of 32 valence electrons for the H3PO4 Lewis structure. When we have an H (or H2 or H3) in front of a polyatomic molecule (like CO3, SO4, NO2, PO4,etc.) we know that it's an acid. This means that the Hydrogen atoms will be attached to the outside of the oxygen molecules.</span>
Leviafan [203]3 years ago
6 0
There are a total of 32 valence electrons for the hp3o4 Lewis structure.
I don't quit understand your question, but I will try to answer it with a picture.

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In which situation are unbalanced forces acting on an object?(1 point)
Alex Ar [27]

Answer:

1. Two people stand on the same side of a large tire. Both people pull the tire with equal force.

2. an object’s ability to not change its motion

3. The car moves forward, while inertia keeps the balloon in place.

4. The unbalanced forces of air resistance and gravity slow the airplane and pull it down.

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7 0
3 years ago
Determine the volume of occupied by 4 moles of carbon dioxide gas at
valentina_108 [34]

Answer:

Vol of 4 moles CO₂(g) at STP = 89.6 Liters

Explanation:

STP

P = 1 Atm

V =

T = 0°C = 273 K

n = 4 moles

R = 0.08206 L·Atm/mol·K

Using Ideal Gas Law PV = nRT => V = nRT/P

V = (4 moles)(0.08206 L·Atm/mol·K)(273 K)/(1 Atm) = 89.6 Liters

5 0
3 years ago
How do I do c2h6 + O2 = CO2 + H2O
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5 0
3 years ago
What’s the definition of ionic solutes?
Sonbull [250]
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6 0
3 years ago
Read 2 more answers
Calculate the concentration of a solution that has 6.7 moles in a volume of 0.6 liters.
Yuri [45]

Answer:

11.2 M

Explanation:

Given data:

Number of moles = 6.7 mol

Volume of solution = 0.6 L

Concentration /Molarity = ?

Solution:

Molarity:

It is number of moles of solute in to per kg or litters of solution. It can be calculated by the following formula.

Molarity = number of moles / Volume in L

Now we will put the values in formula.

Molarity = 6.7 mol / 0.6 L

Molarity = 11.2 mol/L

Molarity = 11.2 M

6 0
4 years ago
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