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3 years ago

Identify the atomic orbitals in the C-C sigma bond in ethyne (acetylene HC-triplebond-CH)

Chemistry

1 answer:

aleksley [76]3 years ago

8 0

Answer:

Explanation:

A sigma bond is formed when a hybrid orbital sp overlaps with another hybrid orbital or with s- or p- orbital

Ethylene has a structural formula of H - C≡ C- H

At the ground state; we have :

C | ⇅ | |↑ | ↑

2s 2p

At the excited state, we have:

C | ↑ | |↑ | ↑ | ↑

the hybrid orbital

C = | ↑ | ↑ |

2sp

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A buffer solution contains 0.479 M NaHCO3 and 0.342 M Na2CO3. Determine the pH change when 0.091 mol HNO3 is added to 1.00 L of

pshichka [43]

Answer:

ΔpH = 0.20

Explanation:

The buffer of HCO₃⁻ + CO₃²⁻ has a pka of 10.2

HCO₃⁻ ⇄ H⁺ + CO₃²⁻

There are 0.479moles of NaHCO₃ and 0.342moles of Na₂CO₃.

Using Henderson-Hasselbalch formula:

pH = pka + log [Base] / [Acid]

pH = 10.2 + log 0.342mol / 0.479mol

pH = 10.05

NaOH reacts with HCO₃⁻ producing CO₃²⁻, thus:

NaOH + HCO₃⁻ → CO₃²⁻ + H₂O + Na⁺

0.091 moles of NaOH produce the same moles of CO₃²⁻ and consume HCO₃⁻. Moles of these species are:

CO₃²⁻: 0.342mol + 0.091mol: 0.433mol

HCO₃⁻: 0.479mol - 0.091 mol: 0.388mol

Using Henderson-Hasselbalch formula:

pH = pka + log [Base] / [Acid]

pH = 10.2 + log 0.433mol / 0.388mol

pH = 10.25

That means change of pH, ΔpH is:

ΔpH = 10.25 - 10.05 = 0.20

I hope it helps!

3 0

2 years ago

What does a pH of 7 say about a solution?

lisov135 [29]

Answer:

Explanation:

it shows that the solution is neutral.

I hope this helps

4 0

3 years ago

How many ions are present in iron 2 oxide

krek1111 [17]

Iron(II) oxide also refers to a family of related non-stoichiometric compounds, which are typically iron deficient with compositions ranging from Fe0.84O to Fe0.95O.

8 0

3 years ago

A 1.5L intraveneous (IV) solution contains 919 grams glucose (C6H12O6). What is the molarity of this solution?

AleksandrR [38]

Answer:

3.4 M

Explanation:

M = grams/molar mass = ans./volume(L)

M = 919/180 = ans./1.5

3 0

3 years ago

Consider the reaction FeO (S) + CO(g) <-----> Fe(s) + CO2(g) for which KP is found to have the following values:

Svetach [21]

Explanation:

$\Delta G^o=-RT\ln K_1$

where,

R = Gas constant = $8.314J/K mol$

T = temperature = $600^oC=[273.15+600]K=873.15 K$

$K_p$ = equilibrium constant at 600°C = 0.900

Putting values in above equation, we get:

$\Delta G^o=-(8.314J/Kmol)\times 873.15 K\times \ln (0.900 )$

$\Delta G^o=764.85 J/mol$

The ΔG° of the reaction at 764.85 J/mol is 764.85 J/mol.

Equilibrium constant at 600°C = $K_1=0.900$

Equilibrium constant at 1000°C = $K_2=0.396$

$T_1=[273.15+600]K=873.15 K$

$T_2=[273.15+1000]K=1273.15 K$

$\ln \frac{K_2}{K_1}=\frac{\Delta H^o}{R}\times [\frac{1}{T_1}-\frac{1}{T_2}]$

$\ln \frac{0.396}{0.900}=\frac{\Delta H^o}{8.314 J/mol K}\times [\frac{1}{873.15 K}-\frac{1}{1273.15 K}]$

$\Delta H^o=-18,969.30 J/mol$

The ΔH° of the reaction at 600 C is -18,969.30 J/mol.

ΔG° = ΔH° - TΔS°

764.85 J/mol = -18,969.30 J/mol - 873.15 K × ΔS°

ΔS° = -22.60 J/K mol

The ΔS° of the reaction at 600 C is -22.60 J/K mol.

$FeO (s) + CO(g)\rightleftharpoons Fe(s) + CO_2(g)$

Partial pressure of carbon dioxide = $p_1=P\times \chi_1$

Partial pressure of carbon monoxide = $p_2=P\times \chi_2$

Where $\chi_1\& \chi_2$ mole fraction of carbon dioxide and carbon monoxide gas.

The expression of $K_p$ is given by:

$K_p=\frac{p_1}{p_2}=\frac{P\times \chi_1}{P\times \chi_2}$

$0.900=\frac{\chi_1}{\chi_2}$

$\chi_1=0.900\times \chi_2$

$\chi_1+\chi_2=1$

$0.9\chi_2+\chi_2=1$

$1.9\chi_2=1$

$\chi_2=\frac{1}{1.9}=0.526$

$\chi_1=1-\chi_2=1-0.526=0.474$

Mole fraction of carbon dioxide at 600°C is 0.474.

6 0

3 years ago