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3 years ago

How many molecules of n2 are in a 200.0 ml container at 780 mmhg and 135∘c?

1 answer:

8 0

By use of ideal gas equation PV= nRT where n is the number of moles,P = pressure, V = volume, R= gas constant (0.08206 L. atm/ mol.k) ant T is the temperature,

to calculate the number of moles(n) =PV/RT

convert ml to L, that is 200/1000= 0.2 L

convert mmHg to atm, that is 780mm hg x 1atm/ 760 mm hg= 1.026 atm

convert temperature to kelvin, that is 135 +273= 408 k
n is therefore= (0.2 x 1.026)/ ( 0.08206 x 408)= 6.129 x10^-3 moles

from avogadro constant 1moles = 6.02 x10^23 molecules what about 6 .129 x10^-3 moles

= ( 6.02 x10^23) x (6.129 x10^-3)/ 1mole = 3.69 x10^21 molecules

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3 years ago

The ionic naming rules

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Identify and name the cation; this is a metal element or polyatomic cation.

Identify and name the anion; this is a nonmetal element. Change the suffix to '-ide,' or use the polyatomic anion name.

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3 years ago

True or false, the four units that must always be used when using the ideal gas law are liters, atm, Kelvin, and grams

maksim [4K]

Answer:

False grams is not used

Explanation:

IDEAL GAS LAW

The ideal gas law states that PV = NkT, where P is the absolute pressure of a gas, V is the volume it occupies, N is the number of atoms and molecules in the gas, and T is its absolute temperature.

It is necessary to use Kelvin for the temperature and it is conventional to use the SI unit of liters for the volume. However, pressure is commonly measured in one of three units: kPa , atm , or mmHg . Therefore, R can have three different values.

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3 years ago

For the reaction 2A(g) â B(g), the equilibrium constant is Kp = 0.76. A reaction mixture initially contains 4.0 atm of gas (PA =

timofeeve [1]

Answer: (a) The reaction mixture will proceed toward products.

Explanation:

Equilibrium constant is defined as the ratio of pressure of products to the pressure of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_p$

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

$2A(g)\rightleftharpoons B(g)$

The expression for $Q_p$ is written as:

$Q_p=\frac{p_B}{(p_A)^2}$

$Q_p=\frac{(2.0)}{(2.0)^2}$

$Q_p=0.5$

$K_p=0.76$

Thus as $K_p>Q_p$ , the reaction will shift towards the right i.e. towards the product side.

7 0

3 years ago

PLS HELP I WILL REWARD MOST BRAINLIEST

kvv77 [185]

Answer:

Actual yield = 138.94 g

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2Na + Cl₂ —> 2NaCl

Next, we shall determine the mass of Na that reacted and the mass of NaCl produced from the balanced equation. This can be obtained as follow:

Molar mass of Na = 23 g/mol

Mass of Na from the balanced equation = 2 × 23 = 46 g

Molar mass of NaCl = 23 + 35.5

= 58.5 g/mol

Mass of NaCl from the balanced equation = 2 × 58.5 = 117 g

SUMMARY:

From the balanced equation above,

46 gof Na reacted to produce 117 g of NaCl.

Next, we shall determine the theoretical yield NaCl. This can be obtained as follow:

From the balanced equation above,

46 gof Na reacted to produce 117 g of NaCl.

Therefore, 57.50 g of Na will react to produce = (57.50 × 117)/46 = 146.25 g of NaCl.

Thus, the theoretical yield of NaCl is 146.25 g

Finally, we shall determine the actual yield of NaCl. This can be obtained as follow:

Percentage yield = 95%

Theoretical yield = 146.25 g

Actual yield =?

Percentage yield = Actual yield / Theoretical yield × 100

95% = Actual yield / 146.25

Cross multiply

Actual yield = 95% × 146.25

Actual yield = 95/100 × 146.25

Actual yield = 0.95 × 146.25

Actual yield = 138.94 g

4 0

3 years ago