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4 years ago

15

When a weak acid (HA) is titrated with sodium hydroxide in the presence of an indicator (Hln), the pH at which a color change is

observed depends on the:

1 answer:

k0ka [10]4 years ago

3 0

Explanation:

the atmosphere and temps

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: Starting with 0.3500 mol CO(g) and 0.05500 mol COCl2(g) in a 3.050-L flask at 668 K, how many moles of Cl2(g) will be present

Mrac [35]

Answer:

The number of moles of Cl₂ present at equilibrium is 3.94x10⁻⁴ moles.

Explanation:

The reaction is:

CO(g) + Cl₂(g) ⇄ COCl₂(g)

The equilibrium constant of the above reaction is:

K = 1.2x10³

To find the moles of Cl₂ present at equilibrium, let's evaluate the reverse reaction:

COCl₂(g) ⇄ CO(g) + Cl₂(g)

The equilibrium constant for the reverse reaction is:

$K_{r} = \frac{1}{1.2 \cdot 10^{3}} = 8.3 \cdot 10^{-4}$

Now, we need to calculate the concentration of CO and COCl₂:

$C_{CO} = \frac{\eta_{CO}}{V} = \frac{0.3500 moles}{3.050 L} = 0.115 M$

$C_{COCl_{2}} = \frac{\eta_{COCl_{2}}}{V} = \frac{0.05500 moles}{3.050 L} = 0.018 M$

Now, from the reaction we have:

COCl₂(g) ⇄ CO(g) + Cl₂(g)

0.018 - x 0.115+x x

The concentration of Cl₂ is:

$K_{r} = \frac{[CO][Cl_{2}]}{[COCl_{2}]}$

$8.3 \cdot 10^{-4} = \frac{(0.115 + x)(x)}{0.018 - x}$

$8.3 \cdot 10^{-4}*(0.018 - x) - (0.115 + x)(x) = 0$

By solving the above equation for x we have:

x = 1.29x10⁻⁴ M = [Cl₂]

Finally, the number of moles of Cl₂ present at equilibrium is:

$\eta_{Cl_{2}} = C_{Cl_{2}}*V = 1.29 \cdot 10^{-4} mol/L*3.050 L = 3.94 \cdot 10^{-4} moles$

Therefore, the number of moles of Cl₂ present at equilibrium is 3.94x10⁻⁴ moles.

I hope it helps you!

8 0

3 years ago

Which feature of nuclear fission reactions allows these reactions to take place in a chain reaction?

adell [148]

the cycle will continue until to fuel is present. that is why chain reaction occurs in a fission reaction

8 0

3 years ago

Read 2 more answers

A chemist measures the amount of iodine solid produced during an experiment. she finds that 1.6 g of iodine solid is produced. c

Yakvenalex [24]

Mass of iodine solid produced = 1.6 g

Iodine solid has a molecular formula : I2

Atomic mass of iodine = 126.904 g/mol

Therefore, molar mass of I2 solid = 2* 126.904 = 253.808 g/mol

Number of moles of a given substance is the ratio of its mass to the molar mass

# moles of I2 solid = mass of I2 solid/molar mass = 1.6 g/253.808 = 0.00630 moles

Hence, the # moles of iodine solid produced is 0.00630 moles

3 0

4 years ago

How many molecules are in 48 grams of oxygen gas?

Alinara [238K]

Answer:

Since oxygen (O) has an atomic mass of 16 g, oxygen gas (O2) has a molecular mass of 2 x 16 = 32 g. We need to convert the given amount of oxygen gas to moles and this can be done by dividing the given mass by the molecular weight of oxygen gas. Hence, moles of oxygen gas = 48 g / 32 g/mole = 1.5 moles.

Explanation:

BARK BARK Hope it helps

PS: CAn doge Have some BEpis He was Good Boy ^m^

4 0

3 years ago

Read 2 more answers

If 0.278g of argon dissolves in 1.5 l of water at 62 bar, what quantity of argon will dissolve at 78 bar

irinina [24]

When P1/P2 = C1/C2

and C is the molarity which = moles/volume

so, P1/P2 = [(mass1/mw)/volume] / [(mass2/mw)/volume]

P1/P2 = (mass1/mw)/1.5L / (mass2/mw)/1.5L

so, Mw and 1.5 L will cancel out:

∴P1/P2 = mass1 / mass2

∴ mass 2 = mass1*(P2 / P1)

= 0.278g * (78 bar / 62 bar)

= 0.35 g

∴ the quantity of argon that will dissolve at 78 bar = 0.35 g

5 0

3 years ago