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4 years ago

Does anyone know how to do common ion effect in chemistry?

Chemistry

1 answer:

pishuonlain [190]4 years ago

7 0

Answer:

no i do not sorry for you

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In a first–order reaction (A → B and rate = k [A]), tripling the concentration of A will have what effect on the reaction rate?

drek231 [11]

Your answer is b just got done doing mine .

3 0

3 years ago

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Charlie the Chemist heats a 62.51 g piece of copper from 22.9°C to 345.0°C. Calculate the amount

Ivanshal [37]

Mass=m=62.51g
Initial temperature=T_i=22.9°C
Final temperature=T_f=345.0°C
Specific heat of copper=0.0920cal/g°C
∆T=T_f-T_i=345-22.9=322.1°C

$\\ \tt\hookrightarrow Q=mc\Delta T$

$\\ \tt\hookrightarrow Q=62.1(0.0920)(322.1)$

$\\ \tt\hookrightarrow Q=1840.22172cal$

$\\ \tt\hookrightarrow Q=1840.222cal$

$\\ \tt\hookrightarrow Q=1840.2cal$

6 0

3 years ago

Oxygen gas, generated by the reaction 2KClO3(s)->2KCl(s)+3O2(g) is collected over water at 27°C in a 1.55 L vessel at a total

KonstantinChe [14]

Answer:

Explanation:

Use Dalton's law and the vapor pressure of water at 23.0 o C to correct the pressure to units of atmoshperes.

PT = Poxygen +Pwater

At 23.0 o C the vapor pressure of water is 21.1 mmHg. (This can be found on a vapor pressure table.)

762 mmHg = Poxygen + 21.1 mmHg

Poxygen = 762 mmHg - 21.1 mmHg

Poxygen =741 mmHg

Convert the corrected pressure to atmospheres.

(741 mmHg) (1 atm / 760 mmHg) = 0.975 atm

Use the ideal gas law to find out how many moles of gas were produced:

PV = nRT (remember to put volume in liters and temperature in Kelvin)

(0.975 atm) (.193 L) = n (.0821 L atm / mol K) (298 K)

n = (0.975 atm) (.193 L) / (.0821 L atm / mol K) (298 K)

n = 7.69 X 10-4 mol

Use the number of moles and the molecular weight of oxygen to find out how many grams of oxygen were collected.

(7.69 X 10-4 mol) (32.0 g / 1 mol) = 2.46 X 10-2 g

4 0

3 years ago

5 pois

schepotkina [342]

The remaining 90% transforms into Hydrogen and Oxygen. The remaining 90% is recombined to maker larger molecules. I think

6 0

3 years ago

If Carl buys a 946 ml bottle of rubbing alcohol, how much of the aqueous solution is water?

Darina [25.2K]

The question is incomplete, here is the complete question:

A bottle of rubbing alcohol having aqueous solution of alcohol contains 70% (v/v) alcohol. If Carl buys a 946 ml bottle of rubbing alcohol, how much of the aqueous solution is water?

<u>Answer:</u> The amount of water present in the given bottle of rubbing alcohol is 283.8 mL

<u>Explanation:</u>

We are given:

Volume of bottle of rubbing alcohol = 946 mL

70% (v/v) alcohol solution

This means that 70 mL of rubbing alcohol is present in 100 mL of solution

Amount of water present in solution = [100 - 70] = 30 mL

Applying unitary method:

In 100 mL of solution, the amount of water present is 30 mL

So, in 946 mL of solution, the amount of water present will be = $\frac{30}{100}\times 946=283.8mL$

Hence, the amount of water present in the given bottle of rubbing alcohol is 283.8 mL

4 0

3 years ago