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2 years ago

A beaker has 0.2 M of Na2SO4. What will be the concentration of sodium and sulfate ions?

Chemistry

1 answer:

netineya [11]2 years ago

7 0

The concentration of sodium and sulphate ions are [ $Na^+$ ] = 0.4 M, [ $SO_4^2-$ ] = 0.2 M

Explanation:

The molar concentration is defined as the number of moles of a molecule or an ion in 1 liter of a solution.

In the given solution, the concentration of the salt sodium sulphate is 0.2M. So, 0.2 moles of sodium sulphate is present in 1 liter of solution.

Assuming 100% dissociation,

1 molecule of sodium sulphate gives 2 ions of sodium and 1 ion of sulphate.

So 0.2 moles of sodium sulphate will give 0.4 moles of sodium ions and 0.2 moles of sulphate ions.

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Gaseous cyclobutene undergoes a first-order reaction to form gaseous butadiene. At a particular temperature, the partial pressur

Gnoma [55]

Answer:

41.3 minutes

Explanation:

Since the reaction is a first order reaction, therefore, half life is independent of the initial concentration, or in this case, pressure.

$t_{1/2}= \frac{0.693}{K}$

So, fraction of original pressure = $\frac{1}{2}^2$

n here is number of half life

therefore, $\frac{1}{8}= \frac{1}{2}^3$

⇒ n= 3

it took 124 minutes to drop pressure to 1/8 of original value, half life = 124/3= 41.3 minutes.

8 0

2 years ago

Read 2 more answers

in a mixture of helium and chlorine, occupying a volume of 12.8 l at 605.6 mmhg and 21.6 oc, it is found that the partial pressu

rodikova [14]

Answer:

Mass of sample = 8.483 g

Explanation:

Given data;

Volume of mixture = 12.8 L

Pressure = 605.6 mmHg ( 605.6 / 760 = 0.797 atm)

Temperature = 21.6 °C (21.6 + 271.15 = 294.8 K)

Partial pressure of chlorine = 143 mmHg ( 143/760 = 0.19 atm)

Solution:

First of all we will determine the number of moles of mixture.

PV = nRT

n = PV/RT

n = 0.797atm × 12.8L / 0.0821 atm. dm³ mol⁻¹ K⁻¹ ×294.8 K

n = 10.202 / 24.2031

n = 0.422 mol

partial pressure of chlorine is 0.19 atm so mole fraction is,

mole fraction = 0.19/0.797

mole fraction = 0.24

moles of chlorine = 0.24 × 0.422 = 0.1013 mol

moles of helium = moles of mixture - moles of chlorine

moles of helium = 0.422 - 0.1013

moles of helium = 0.3207 mol

Mass of chlorine = moles × molar mass

Mass of chlorine = 0.1013 mol × 71 g/mol

Mass of chlorine = 7.2 g

Mass of helium = moles × molar mass

Mass of helium = 0.3207 mol × 4 g/mol

Mass of helium = 1.283 g

Mass of sample = mass of chlorine + mass of helium

Mass of sample = 7.2 g + 1.283 g

Mass of sample = 8.483 g

5 0

2 years ago

Air containing 20.0 mol% water vapor at an initial pressure of 1 atm absolute is cooled in a 1- liter sealed vessel from 200°C t

chubhunter [2.5K]

Answer:

This solution is quite lengthy

Total system = nRT

n was solved to be 0.02575

nH20 = 0.2x0.02575

= 0.00515

Nair = 0.0206

PH20 = 0.19999

Pair = 1-0.19999

= 0.80001

At 15⁰c

Pair = 0.4786atm

I used antoine's equation to get pressure

The pressure = 0.50

2. Moles of water vapor = 0.0007084

Moles of condensed water = 0.0044416

Grams of condensed water = 0.07994

Please refer to attachment. All solution is in there.

6 0

2 years ago

Who might benefit financially the most from the EPA’s claim? restaurants that use C-8-coated cookware cookware manufacturers who

kondor19780726 [428]

Cookware manufacturers who make pans out of steel only because if C-8 is discontinued then people would have no choice but to buy steel pans. The steel pan manufacturers would in return receive a lot of money

8 0

2 years ago

Read 2 more answers

The burning of 80.3 g of SiH4 at constant pressure gives off 3790 kJ of heat. Calculate △H for this reaction. SiH4(g) + 2O2(g) ⟶

Trava [24]

Answer : The value of ΔH for this reaction is, -1516 kJ/mol

Explanation :

First we have to calculate the moles of $SiH_4$

$\text{Moles of }SiH_4=\frac{\text{Mass of }SiH_4}{\text{Molar mass of }SiH_4}$

$\text{Moles of }SiH_4=\frac{80.3g}{32.12g/mol}$

$\text{Moles of }SiH_4=2.5mol$

Now we have to calculate the ΔH for this reaction.

As, 2.5 mole of $SiH_4$ react to gives heat = -3790 kJ

So, 1 mole of $SiH_4$ react to gives heat = $-\frac{3790kJ}{2.5mol}$

= -1516 kJ/mol

Therefore, the value of ΔH for this reaction is, -1516 kJ/mol

7 0

2 years ago