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2 years ago

I really need help with b. Please help

Chemistry

1 answer:

fiasKO [112]2 years ago

8 0

Answer:

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Explanation:

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How many significant figures are in 6.00 in

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Answer:

Explanation:

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4 years ago

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What is the pOH of a 2.6 x 10-6 M H+ solution?

melomori [17]

Answer:

Approximately $8.41$ (assuming that the solution is at $\rm 25^\circ C$ , under which $K_{\rm w} = 10^{-14}$ .)

Explanation:

Let ${\rm [H^{+}]}$ and ${\rm [OH^{-}]}$ denote the concentration of $\rm H^{+}$ and $\rm OH^{-}$ respectively.

Let $K_{\rm w}$ denote the self-ionization constant of water. The exact value of $K_{\rm w}\!$ depends on the temperature of the solution. $K_{\rm w} =10^{-14}$ at $\rm 25^\circ C$ .

The product of ${\rm [H^{+}]}$ and ${\rm [OH^{-}]}$ in a solution (with $\rm M$ , or moles per liter, as the unit) is supposed to be equal to the $K_{\rm w}$ value of that solution at the corresponding temperature. In other words:

${\rm [H^{+}]} \cdot {\rm [OH^{-}]} = K_{\rm w}$ .

Rearrange to obtain an expression for ${[\rm OH^{-}]}$ :

$\begin{aligned}{\rm [OH^{-}]} &= \frac{K_{\rm w}}{[\rm H^{+}]}\end{aligned}$ .

Assume that the solution in this question is at $\rm 25^\circ C$ (for which $K_{\rm w} =10^{-14}$ .) For this solution:

$\begin{aligned}{\rm [OH^{-}]} &= \frac{K_{\rm w}}{[\rm H^{+}]} \\ &= \frac{10^{-14}}{2.6 \times 10^{-6}}\approx 3.85\times 10^{-9}\; \rm M\end{aligned}$ .

Hence, the $\rm pOH$ of this solution would be:

$\begin{aligned}\rm pOH &= -\log_{10}{\rm [OH^{-}]} \\&\approx -\log_{10} (3.85 \times 10^{-9}) \approx 8.41 \end{aligned}$ .

3 0

3 years ago

Calculate the density in g/l of co2 gas at 27 Celsius and 0.500 atm pressure

lesya692 [45]

Answer:

The density of CO₂ gas at 27 Celsius and 0.500 atm is 0.89 $\frac{grams}{L}$

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P*V = n*R*T Equation (A)

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.

Density allows you to measure the amount of mass in a given volume of a substance. So density is defined as the quotient between the mass of a body and the volume it occupies:

$density=\frac{mass}{volume}$

Being the molar mass of a substance the mass contained in one mole of said substance, the number of moles can be expressed as:

$n=\frac{mass}{molar mass}$ Equation (B)

Replacing in Equation (A):

P*V= $\frac{mass}{molar mass}$ *R*T

Solving to get the definition of density expressed in the equation, you get:

$density=\frac{mass}{V} =\frac{P*molar mass}{R*T}$

Being:

P=0.500 atm
Molar mass CO₂= 44 g/mole

R= 0.082 $\frac{atm*L}{mole*K}$

T= 27 C= 300 K (being 0 C=273 K)

and replacing:

$density=\frac{mass}{V} =\frac{0.500 atm*44 \frac{g}{mole} }{0.082 \frac{atm*L}{mole*K} *300 K}$

you get:

density= 0.89 $\frac{grams}{L}$

The density of CO₂ gas at 27 Celsius and 0.500 atm is 0.89 $\frac{grams}{L}$

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4 years ago

What volume of air contains 10.0g of oxygen gas at 273 k and 1.00 atm?

VARVARA [1.3K]

12.3g 02times1 mol 02/32.0 g 02=mol 02
.38mol/x=20.95/100
x=1.8mol air...

PV=nRT

101.3kPa times V =1.8 mol times 8.31[kPa *L]/{k*mol}*273k
V=40.3Lair

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3 years ago

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If sodium (Na) bonds with chlorine (Cl), which statement is true?

Ray Of Light [21]

Answer:

First option is the correct answer

Explanation:

An electron is transferred from sodium to chlorine and an ionic bond is formed.

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3 years ago

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