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slava [35]
3 years ago
9

What pressure is required to achieve a co2 concentration of 7.90×10−2 m at 20∘c?

Chemistry
1 answer:
Savatey [412]3 years ago
7 0

Answer:-  1.90 atm

Solution:- It is based on combined gas law equation, PV = nRT

In this equation, P is pressure, V is volume, n is moles of gas, R is universal gas constant and T is kelvin temperature.

If we divide both sides by V then:

P=\frac{nRT}{V}

We know that, molarity is moles per liter. So, in the above equation we could replace \frac{n}{V} by molarity, M of the gas. The equation becomes:

P = MRT

T = 20 + 273 = 293 K

M = 7.9*10^-^2

Let's plug in the values in the equation:

P = (7.9*10^-^2)(0.0821)(293)

P = 1.90 atm

So, the pressure of the gas is 1.90 atm.

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To indicate the pH of a substance, one can use a dye that is both an acid and that appears as different colors in its protonated
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Answer:

<em>The pH of the solution is 7.8</em>

Explanation:

The concentration of the solution is 0.001M and  the dye could be in its protonated and deprotonated forms. If the concentration of the protonated form [HA] is 0.0002 M the concentration of the deprotonated form will be the subtraction between the concentration of the bye and the concentration of the protonated form:

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3 years ago
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yanalaym [24]

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