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vesna_86 [32]
3 years ago
11

I need help with this i'm really dumb. Balance p4+o2 ----> p4o10

Chemistry
1 answer:
kogti [31]3 years ago
4 0

Answer:

P4 + 5O2 → P4O10

Explanation:

White Phosphorus - P4

Dioxygen - O2

Tetraphosphorus Decaoxide - P4O10

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The flame symbol represents which of the following hazards?
mart [117]
Fire Hazard would be the correct answer
4 0
3 years ago
Read 2 more answers
Calculate the vapor pressure of a solution containing 25.2 gg of glycerin (C3H8O3)(C3H8O3) in 124 mLmL of water at 30.0 ∘C∘C. Th
alexgriva [62]

Answer:

29.256 torr.

Explanation:

Number of moles

Glycerin:

Molecular weight of glycerin = (12*3) + (1*8) + (16*3)

= 36 + 8 + 48

= 92 g/mol

Number of moles = mass/molar mass

= 25.2/92

= 0.274 mol

Water:

Converting g/ml to g/l,

1000 ml = 1 l

= 1 g/ml * 1000 ml/1l

= 1000 g/l

Mass = (density * volume)

= 1000*0.124

= 124 g.

Molar mass of water = (1*2) + 16

= 18 g/mol

Number of moles = mass /molar mass

= 126/18

= 6.89 mol

P°solution = xsolvent * P°solvent

Where,

xwater = xsolvent = mole fraction of water.

Mole fraction is defined as the number of moles of a component of a solution divided by the total number of moles present in that solution.

xwater = mole of water/total mole of solution

Total mole = 6.89 + 0.274

= 7.164 moles

xwater = 6.89/7.164

= 0.962

P°solution = xsolvent * P°solvent

P°solution = 31.8 * 0.962

= 29.256 torr

6 0
2 years ago
"Inert" xenon actually forms many compounds, especially with highly electronegative fluorine. The ΔH° values for xenon difluorid
svp [43]

The average bond energy of the Xe¬F bonds in each fluoride is 132kJ/mol.

Given:

ΔH° of xenon difluoride (XeF2) = -105 kJ/mol

ΔH° of xenon tetrafluoride (XeF4)= -284 kJ/mol

ΔH° of xenon hexafluoride (XeF6) = -402 kJ/mol

The bond energy of Xe-F in XeF2 can be calculated as follows,

As we know that

ΔH° = ΔH°(bond formed) + ΔH°(bond broken)

The chemical reaction for the formation of XeF2 can be written in such a way,

Xe (g) + F2 (g) → XeF2 (g)

= [1 mol F2 (159 kJ/mol)] + [2(-Xe-F)] - 105 kJ/mol

= 159 kJ/mol + 2(-Xe-F) - 264 kJ/mol

= 2(-Xe-F)

Xe-F = 132 kJ/mol

Thus, we concluded that the average bond energy of the Xe¬F bonds in each fluoride is 132kJ/mol.

learn more about bond energy:

brainly.com/question/11653058

#SPJ4

3 0
1 year ago
What is the name of the compound CaCo3​
ddd [48]
The compound is calcium carbonate
4 0
2 years ago
Determine which elements or compounds are products in the<br> follow reaction equation:
Anna71 [15]

Answer: D is the answer since it is the product of this equation

Explanation: HOPE I AM RIGHT AND IT HELPS!!!

need more explanation feel free to comment in the comment box

4 0
3 years ago
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