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3 years ago

1. The volume of a gas is 10.0 liters and its temperature is 1500 K. If the temperature is

Chemistry

1 answer:

cupoosta [38]3 years ago

5 0

Answer:

5 L

Explanation:

So this problem refers to Charles's law. You would use this formula..

$\frac{V_{I} }{T_{I} } = \frac{V_{F} }{T_{F} }$ (Initial volume / Initial Temperature) = (Final volume / Final Temperature)

For your problem, it would look like this...

$\frac{10L}{1500k} = \frac{V_{F} }{750k}$

You would cross multiply and your answer would be 5L.

To reassure yourself that the answer is correct, Charles law states that the Volume and the Temperature are directly proportional. Meaning if your temperature is decreasing, your volume <u>has</u> to decrease.

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For a process Arightwards harpoon over leftwards harpoonB, at 25 °C there is 10% of A at equilibrium while at 75 °C, there is 80

Lostsunrise [7]

This question is describing the following chemical reaction at equilibrium:

$A\rightleftharpoons B$

And provides the relative amounts of both A and B at 25 °C and 75 °C, this means the equilibrium expressions and equilibrium constants can be written as:

$K_1=\frac{90\%}{10\%}=9\\\\K_2=\frac{20\%}{80\%} =0.25$

Thus, by recalling the Van't Hoff's equation, we can write:

$ln(K_2/K_1)=-\frac{\Delta H}{R}(\frac{1}{T_2} -\frac{1}{T_1} )$

Hence, we solve for the enthalpy change as follows:

$\Delta H=\frac{-R*ln(K_2/K_1)}{(\frac{1}{T_2} -\frac{1}{T_1} ) }$

Finally, we plug in the numbers to obtain:

$\Delta H=\frac{-8.314\frac{J}{mol*K} *ln(0.25/9)}{[\frac{1}{(75+273.15)K} -\frac{1}{(25+273.15)K} ] } \\\\\\\Delta H=4,785.1\frac{J}{mol}$

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3 years ago

1 mole solution of NaCl contains

Mamont248 [21]

Answer:

If you dissolve 58.44g of NaCl in a final volume of 1 liter, you have made a 1M NaCl solution, a 1 molar solution.

Explanation:

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3 years ago

A gas occupies a 1.5 L container at 25 degrees Celsius and 2.0 atm. If the gas is transferred to a 3.0 L container at the same t

harkovskaia [24]

To solve this we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 =P2V2

P2 = P1 x V1 / V2

P2 = 2.0 x 1.5 / 3

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3 years ago

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How many grams of MnCl2 need to be added to 5 liters of water to make a 0.25 M solution?

damaskus [11]

Answer:

I think it is 860 g MG Cl2

Explanation:

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3 years ago

Given 700 ml of oxygen at 7 ºC and 80.0 cm Hg pressure, what volume does it take at 27 ºC and 50.0 cm Hg pressure?

katen-ka-za [31]

Answer:

I think that it might be 2.7

Explanation:

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3 years ago