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Kobotan [32]
3 years ago
14

Based on molecular orbital theory, the bond orders of the H—H bonds in H 2 , H 2 + , and H 2 - are _________, respectively

Chemistry
1 answer:
vodka [1.7K]3 years ago
4 0

Answer:

H2-1

H2+-1/2

H22- zero

Explanation:

Bond order= Bonding electrons-antibonding electrons/2

In H2, there are two bonding electrons and no antibonding electrons. In H2+ there is only one bonding electron and no antibonding electron while in H22- there are two bonding and two antibonding electrons respectively.

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Assume that you have a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if you do the f
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Answer:

A. The pressure will increase 4 times. P₂ = 4 P₁

B. The pressure will decrease to half its value. P₂ = 0.5 P₁

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Explanation:

Initially, we have n₁ moles of a gas that occupy a volume V₁ at temperature T₁ and pressure P₁.

<em>What would happen to the gas pressure inside the cylinder if you do the following?</em>

<em />

<em>Part A: Decrease the volume to one-fourth the original volume while holding the temperature constant. Express your answer in terms of the variable P initial.</em>

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P₁ . V₁ = P₂ . V₂

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P₁ = P₂ . 0.25

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<em>Part B: Reduce the Kelvin temperature to half its original value while holding the volume constant. Express your answer in terms of the variable P initial.</em>

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\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}}\\\frac{P_{1}}{T_{1}} =\frac{P_{2}}{0.5T_{1}}\\\\P_{2}=0.5P_{1}

<em>Part C: Reduce the amount of gas to half while keeping the volume and temperature constant. Express your answer in terms of the variable P initial.</em>

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P_{1}=\frac{n_{1}.R.T_{1}}{V_{1}}

P₂ in terms of the ideal gas equation is:

P_{2}=\frac{n_{2}.R.T_{1}}{V_{1}}=\frac{0.5n_{1}.R.T_{1}}{V_{1}}=0.5P_{1}

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For the reaction represented by the equation 
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