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nikklg [1K]
3 years ago
15

How many bonds and lone pairs are in the molecule SIH4?

Chemistry
1 answer:
lesantik [10]3 years ago
6 0

Answer:

there are no valence electrons left over, so the molecule has four bond pairs and no lone pairs.

Explanation:

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Determine the value of the equilibrium constant, Kgoal, for the reaction C(s)+12O2(g)+H2(g)⇌12CH3OH(g)+12CO(g), Kgoal=? by makin
Licemer1 [7]

Answer:

1.71x10²⁷

Explanation:

If we sum 1/2 of (3) + 1/2 of (1):

1/2 (3.) C(s) + 1/2O₂(g) ⇌ CO(g), K₃ = √2.10×10⁴⁷  = 4.58x10²³

1/2 (1)   1/2CO₂(g) + 3/2H₂(g) ⇌ 1/2CH₃OH(g) + 1/2H₂O(g), K₁ = √1.40×10² = 11.8

C(s) + 1/2O₂(g) +<u> 1/2CO₂(g) </u>+<u> 3/2H₂(g</u>) ⇌ 1/2CH₃OH(g) + <u>1/2H₂O(g)</u> + <u>CO(g)</u>

K' = 4.58x10²³ * 11.8 = 5.42x10²⁴

+1/2 (2):

<u>1/2 CO(g)</u> +<u> 1/2H₂O(g)</u> ⇌<u> 1/2CO₂(g)</u> + <u>1/2H₂</u> (g), K = √1.00×10⁵ = 316.2

C(s) + 1/2O₂(g) + H₂(g) ⇌ 1/2 CHO₃H(g) + 1/2CO(g)

K'' = 5.42x10²⁴* 316.2 =

<h3>1.71x10²⁷</h3>

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3 years ago
What do us, humans and sharks have in common
Yuki888 [10]
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What is the stable ion of cesium
Sauron [17]

Answer:

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Explanation:

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Dawson decided he would be Dawson and play with a flammable gas. He needs to know how many moles of gas it takes to occupy 210 L
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According to ideal gas equation, 0.5186 moles of gas are required to occupy 210 L at a pressure of 5.4 atmospheres and a temperature of 263 K.

<h3>What is ideal gas equation?</h3>

The ideal gas equation is a equation which is applicable in a hypothetical state of an ideal gas.It is a combination of Boyle's law, Charle's law,Avogadro's law and Gay-Lussac's law . It is given as, PV=nRT where R= gas constant whose value is 8.314.The law has several limitations.

Substituting the given values in the given equation, n= 5.4×210/8.314×263=0.5186 moles

Thus there are 0.5186 moles occupying  210 L at a pressure of 5.4 atmospheres and a temperature of 263 K.

Learn more about ideal gas equation,here:

brainly.com/question/28837405

#SPJ1

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In order to be a chemical reaction matter must be used up or destroyed
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The atoms are rearranged...
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