Which of the following is the conjugate base of phosphoric acid? *

koban [17]

<span><span>An erection that will not go away (priapism).
S</span><span>udden vision loss in one or both eyes
</span>Sudden hearing decrease or hearing loss.</span>

7 0

3 years ago

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Select all of the items that are true about a sample of water vapor at 101°C as it cools.

Dvinal [7]

<h3><u>Answer;</u></h3>

A) Its temperature will fall continuously until it condensed into a liquid.

<h3><u>Explanation</u>;</h3>

<em><u>Steam or water vapor is the gaseous state of liquid water. When water vapor above a temperature of 100 degrees Celsius is cooled, the temperature falls continuously, and it undergoes condensation at a temperature of 100 degrees Celsius and turns into liquid water.</u></em>
The change of state from gaseous to liquid state occurs as a result of latent heat of vaporization that the water vapor carries.

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3 years ago

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If a certain gas occupies a volume of 10. L when the applied pressure is 5.0 atm , find the pressure when the gas occupies a vol

lorasvet [3.4K]

Answer:

20L is the new volume

Explanation:

In this case, moles and T° from the gas remain constant. This is the formula we must apply, to solve this:

P₁ . V₁ = P₂ . V₂

5 atm . 10 L = P₂ . 2.5L

P₂ = (5 atm . 10 L) / 2.5L →20L

5 0

3 years ago

Hydrogen is manufactured on an industrial scale by this sequence of reactions: Write an equation that gives the overall equilibr

RideAnS [48]

The question is incomplete. The complete question is :

Hydrogen is manufactured on an industrial scale by this sequence of reactions:

$CH_3(g) + H_2O(g) \rightleftharpoons CO(g) + 3H_2(g ) \ \ \ \ \ \ \ \ \ \ K_1$

$CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g) \ \ \ \ \ \ \ \ \ \ \ \ K_2$

The net reaction is :

$CH_4(g) + 2H_2O(g) \rightleftharpoons CO_2(g) + 4H_2(g) \ \ \ \ \ \ \ \ \ K$

Write an equation that gives the overall equilibrium constant $K$ in terms of the equilibrium constants $K_1$ and $K_2$ . If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator.

Solution :

$CH_3(g) + H_2O(g) \rightleftharpoons CO(g) + 3H_2(g ) \ \ \ \ \ \ \ \ \ \ K_1$

$K_1 = \frac{[CO][H_2]^3}{[CH_4][H_2O]}$ ...............(1)

$CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g) \ \ \ \ \ \ \ \ \ \ \ \ K_2$

$K_2 = \frac{[CO_2][H_2]}{[CO][H_2O]}$ ...................(2)

$CH_4(g) + 2H_2O(g) \rightleftharpoons CO_2(g) + 4H_2(g) \ \ \ \ \ \ \ \ \ K$

$K=\frac{[CO_2][H_2]^4}{[CH_4][H_2O]^2}$

On multiplication of equation (1) and (2), we get

$K_1 \times K_2=\frac{[CO][H_2]^3}{[CH_4][H_2O]} \times \frac{[CO_2][H_2]}{[CO][H_2O]}$

$K_1K_2=\frac{[CO_2][H_2]^4}{[CH_4][H_2O]^2}$ .................(4)

Comparing equation (3) and equation (4), we get

$K=K_1K_2$

4 0

3 years ago

how many moles of iodine should be added to 750 grams of carbon tetrachloride to prepare a 0.24 m solution

aleksley [76]

Answer:

0.18 mol

Explanation:

Given data

Mass of carbon tetrachloride (solvent): 750 g

Molality of the solution: 0.24 m

Moles of iodine (solute): ?

Step 1: Convert the mass of the solvent to kilograms

We will use the relationship 1 kg = 1,000 g.

$750g \times \frac{1kg}{1,000g} =0.750kg$

Step 2: Calculate the moles of the solute

The molality is equal to the moles of solute divided by the kilograms of solvent. Then,

$m = \frac{moles\ of\ solute }{kilograms\ of\ solvent} \\moles\ of\ solute = m \times kilograms\ of\ solvent = \frac{0.24mol}{kg} \times 0.750kg = 0.18 mol$

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3 years ago

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