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3 years ago

What is the partial pressure of C? atm C

Chemistry

1 answer:

s344n2d4d5 [400]3 years ago

8 0

The partial pressure of carbon is 45 mm Hg.

Explanation:

The partial pressure of carbon dioxide is referred as the amount of carbon dioxide present in venous or arterial blood. It acts as a ventilation in the lungs.
There is a formula for measuring partial pressure . As we know total pressure means summation of the pressure of all the gases included .
To find partial pressure we need- total pressure* fraction of mole of that gas. The partial pressure of CO2 is more because it carries deoxygenated blood from the whole body towards the lungs.

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Write the overall, balanced molecular equation and indicate which element is oxidized and which is reduced for the following rea

galina1969 [7]

Answer:

Cd(s) + AgNO₃(aq) → Cd(NO₃)₂ (aq) + Ag(s)

Oxidized: Cd

Reduced: Ag

Explanation:

Cd(s) + AgNO₃(aq) → Cd(NO₃)₂ (aq) + Ag(s)

Cd → Cd²⁺ + 2e⁻ Half reaction oxidation

1e⁻ + Ag⁺ → Ag Half reaction reduction

Ag changed oxidation number from +1 to 0

Cd changed oxidation number from 0 to +2

Let's ballance the electrons

( Cd → Cd²⁺ + 2e⁻ ) .1

( 1e⁻ + Ag⁺ → Ag ) .2

Cd + 2e⁻ + 2Ag⁺ → 2Ag + Cd²⁺ + 2e⁻

Finally the ballance equation is:

Cd(s) + 2AgNO₃(aq) → Cd(NO₃)₂ (aq) + 2Ag(s)

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3 years ago

In the laboratory, a general chemistry student measured the pH of a 0.529 M aqueous solution of phenol (a weak acid), C6H5OH to

Artyom0805 [142]

Answer:

The dissociation constant of phenol from given information is $9.34\times 10^{-11}$ .

Explanation:

The measured pH of the solution = 5.153

$C_6H_5OH\rightarrow C_6H_5O^-+H^+$

Initially c

At eq'm c-x x x

The expression of dissociation constant is given as:

$K_a=\frac{[C_6H_5O^-][H^+]}{[C_6H_5OOH]}$

Concentration of phenoxide ions and hydrogen ions are equal to x.

$pH=-\log[x]$

$5.153=-\log[x]$

$x=7.03\times 10^{-6} M$

$K_a=\frac{x\times x}{(c-x)}=\frac{x^2}{(c-x)}=\frac{(7.03\times 10^{-6} M)^2}{ 0.529 M-7.03\times 10^{-6} M}$

$K_a=9.34\times 10^{-11}$

The dissociation constant of phenol from given information is $9.34\times 10^{-11}$ .

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pickupchik [31]

Answer:

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Explanation:

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trasher [3.6K]

Answer:

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