Ask question

Ask question

All categories

stealth61 [152]

3 years ago

14

) The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing

the water levels inside and outside the gas-collection tube, as shown in the diagram below. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr . (i) The pressure inside the tube due to the H2(g)

1 answer:

Oksana_A [137]3 years ago

3 0

Answer:

P (H₂) = 741 torr

Explanation:

Let's begin by listing out the given parameters:

Temperature (water) = 298 K, volume = 45.6 mL,

atmospheric pressure, P (total) = 765 torr, vapor pressure of water, P (H₂O) = 24 torr

To get the pressure of inside the tube, P (H₂), we apply Dalton's Law of Partial Pressure and we have:

P (total) = P (H₂) + P (H₂O)

P (total) = 765 torr, P (H₂O) = 24 torr

P (H₂) = P (total) - P (H₂O) = 765 - 24

P (H₂) = 741 torr

It therefore becomes clear that the pressure of H₂(g) is 741 torr

You might be interested in

SCIENCE HELP !!!! 10 POINTS

stich3 [128]

Im working on science too!! I would help you but the attachment isn't pulling up..

5 0

3 years ago

Calculate either [ H 3 O + ] or [ OH − ] for each of the solutions.

STALIN [3.7K]

Answer: Solution A : $[H_3O^+]=0.300\times 10^{-7}M$

Solution B : $[OH^-]=0.107\times 10^{-5}M$

Solution C : $[OH^-]=0.177\times 10^{-10}M$

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration and pOH is calculated by taking negative logarithm of hydroxide ion concentration.

$pH=-\log[H_3O^+]$

$pOH=-log[OH^-}$

$pH+pOH=14$

$[H_3O^+][OH^-]=10^{-14}$

a. Solution A: $[OH^-]=3.33\times 10^{-7}M$

$[H_3O^+]=\frac{10^{-14}}{3.33\times 10^{-7}}=0.300\times 10^{-7}M$

b. Solution B : $[H_3O^+]=9.33\times 10^{-9}M$

$[OH^-]=\frac{10^{-14}}{9.33\times 10^{-9}}=0.107\times 10^{-5}M$

c. Solution C : $[H_3O^+]=5.65\times 10^{-4}M$

$[OH^-]=\frac{10^{-14}}{5.65\times 10^{-4}}=0.177\times 10^{-10}M$

7 0

3 years ago

The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl et

Alexxx [7]

<u>Answer:</u> The vapor pressure of solution is 459.17 mmHg

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

<u>For testosterone:</u>

Given mass of testosterone = 7.752 g

Molar mass of testosterone = 288.4 g/mol

Putting values in equation 1, we get:

$\text{Moles of testosterone}=\frac{7.752g}{288.4g/mol}=0.027mol$

<u>For diethyl ether:</u>

Given mass of diethyl ether = 208.0 g

Molar mass of diethyl ether = 74.12 g/mol

Putting values in equation 1, we get:

$\text{Moles of diethyl ether}=\frac{208.0g}{74.12g/mol}=2.81mol$

Mole fraction of a substance is calculated by using the equation:

$\chi_A=\frac{n_A}{n_A+n_B}$

$\chi_{\text{testosterone}}=\frac{n_{\text{testosterone}}}{n_{\text{testosterone}}+n_{\text{diethyl ether}}}$

$\chi_{\text{testosterone}}=\frac{0.027}{0.027+2.81}\\\\\chi_{\text{testosterone}}=0.0095$

The formula for relative lowering of vapor pressure will be:

$\frac{p^o-p_s}{p^o}=i\times \chi_{\text{solute}}$

where,

$p^o$ = vapor pressure of solvent (diethyl ether) = 463.57 mmHg

$p^s$ = vapor pressure of the solution = ?

i = Van't Hoff factor = 1 (for non electrolytes)

$\chi_{\text{solute}}$ = mole fraction of solute (testosterone) = 0.0095

Putting values in above equation, we get:

$\frac{463.57-p^s}{463.57}=1\times 0.0095\\\\p^s=459.17mmHg$

Hence, the vapor pressure of solution is 459.17 mmHg

7 0

3 years ago

What are the two most common elements in the entire universe

g100num [7]

Answer: Hydrogen and Helium

Explanation: Hydrogen is made from from one proton and one electron, making them one of the simplest forms of elements in the universe. Combining hydrogen atoms creates helium, the second most common element in the Universe.

5 0

3 years ago

Read 2 more answers

How much mass do 3.4 moles of silver contain?

tensa zangetsu [6.8K]

367.2 g of silver

Explanation:

To find the mass of a substance knowing the number of moles we use the following formula:

number of mole = mass / molecular weight

In the case of silver we use the atomic weight of 108 g/mole.

mass = number of moles × molecular weight

mass of silver = 3.4 moles × 108 g/mole

mass of silver = 367.2 g

Learn more about:

moles

brainly.com/question/2293005

#learnwithBrainly

5 0

3 years ago