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2 years ago

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Calculate the ph of a solution that is 0.6 m in sodium acetate and 0.2 m in acetic acid. ka = 1.8 × 10−5 for acetic acid. 1. ph

= 4.3 2. ph = 4.7 3. ph = 5.2 4. ph = 2.7 5. ph = 5.6

1 answer:

Arte-miy333 [17]2 years ago

4 0

0.53 x 200ml = 106 ml of the pH 9.0 buffer + 94 ml of the pH 10 buffer gives the desired solution
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65g of nitric acid are produced in a reaction. 2.5g of platinum are added to the reaction vessel at the start of the reaction to

AysviL [449]

Answer:

2.5 g of platinum

Explanation:

Recall that a catalyst is a specie added to a reaction system to increase the rate of reaction. A catalyst does not participate in the chemical reaction hence it remains unchanged at the end of the chemical reaction. A catalyst merely provides an alternative reaction pathway by lowering the activation energy of the reaction system. Hence a catalysed reaction usually proceeds faster with less energy requirement than the uncatalysed reaction.

Since the catalyst does not participate in the reactions and remains unchanged at the end of the reaction, the mass of platinum will remain the same (2.5g). The mass can only change if a specie participates in the chemical reaction. Hence the answer.

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Are all the molecules in the picture the same?

Dvinal [7]

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There is no picture.

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Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°

Pavel [41]

Answer:

PNO₂ = 0.49 atm

PN₂O₄ = 0.45 atm

Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that involves the density (ρ = m/V).

PV = nRT

n = m/M (m is the mass, and M the molar mass)

$PV = \frac{m}{M}RT$

$PxM = \frac{m}{V}RT$

PxM = ρRT

ρ = PxM/RT

With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

$2.7 = \frac{0.94xMavg}{0.082x289}$

0.94Mavg = 63.9846

Mavg = 68.0687 g/mol

The molar mass of N is 14 g/mol and of O is 16 g/mol, than $M_{NO2} = 46$ g/mol and $M_{N2O4} = 96$ g/mol. Calling y the molar fraction:

$Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}$

And,

$y_{NO2} + y_{N2O4} = 1$

$y_{N2O4} = 1 - y_{NO2}$

So,

$68.0687 = 46y_{NO2} + 92x(1 - y_{NO2})$

$68.0687 - 92 = 46y_{NO2} - 92y_{NO2}$

$46y_{NO2} = 23.9313$

$y_{NO2} = 0.52$

$y_{N2O4} = 0.48$

The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

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2 years ago

When you apply heat energy to a substance, where does the energy go? Think about the law of conservation of energy.

MAVERICK [17]

The energy is transformed into kinetic energy which makes the substance to move. The law of conservation of energy which is the first law of thermodynamics states that in a closed system energy can neither be created nor destroyed but can change from one form to another

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2 years ago

The volume of a gas is 36.0 ml at 10.0°c and 4.50 atm. at what temperature (°c) will the gas have a pressure of 3.50 atm and a v

galben [10]

Using the combined gas law, where PV/T = constant, we first solve for PV/T for the initial conditions: (4.50 atm)(36.0 mL)/(10.0 + 273.15 K) = 0.57213.
Remember to use absolute temperature.
For the final conditions: (3.50 atm)(85.0 mL)/T = 297.5/T
Since these must equal, 0.57213 = 297.5/T
T = 519.98 K
Subtracting 273.15 gives 246.83 degC.

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2 years ago