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Ludmilka [50]
3 years ago
7

The nighttime and daytime temperatures on Mercury are 13 K and 683 K respectively. The melting point and boiling point of sulfur

is 246°F and 832°F. Which of the following statements is true? On Mercury sulfur exists
a. only in the liquid state.
b. only in the solid state.
c. as both a liquid and a gas.
d. as both a liquid and a solid
Chemistry
1 answer:
gizmo_the_mogwai [7]3 years ago
4 0

Answer: Option (d) is the correct answer.

Explanation:

Converting Fahrenheit into kelvin as follows.

           \frac{5}{9} \times (^{o}F - 32) + 273.15

So, 246^{o}F will be converted into kelvin as follows.

            \frac{5}{9} \times (246^{o}F - 32) + 273.15

                = 392.039 K

Also, 832^{o}F will be converted into kelvin as follows.

             \frac{5}{9} \times (832^{o}F - 32) + 273.15                                      

                = 717.594 K

As 13 K is the temperature at night time. So, it means sulfur will exist as a solid at this time because melting point of sulfur is 392.039 K.

Whereas 683 K is the temperature during day time. Hence, it means sulfur will exist in liquid state because its boiling point is 717.594 K.

Thus, we can conclude that on mercury, sulfur exists as both a liquid and a solid.

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What volume of water vapor would be produced from the combustion of 815.74 grams of propane (C3H8) with 1,006.29 grams of oxygen
d1i1m1o1n [39]

3940.2 is the volume of water vapour that would be produced from the combustion of 815.74 grams of propane (C_3H_8) with 1,006.29 grams of oxygen gas, under a pressure of 1.05 atm and a temperature of 350. degrees C.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Stoichiometric calculations:

C_3H_8(g) + 5 O_2(g)→ 3 CO_2(g) + 4 H_2O(g)

From the equation of the reaction, the mole ratio of propane to oxygen is 1:5.

Mole of 815.74 grams of propane = \frac{ 815.74}{44.1 }

Mole of 815.74 grams of propane = 18.49750567 moles

Mole of  1,006.29 grams of oxygen =\frac{ 1,006.29}{32 }

Mole of  1,006.29 grams of oxygen = 31.4465625 moles

Going by the mole ratio, it appears propane is limiting while oxygen is in excess.

From the equation, 1 mole of propane produces 4 moles of water vapour. Thus, the equivalent mole of water vapour will be:

18.49750567 moles x 4 = 73.99 moles.

Using the ideal gas equation:

PV = nRT

v = (73.99  x 0.08206 x 623) ÷ 0.96

v =  3940.2

Hence, 3940.2 is the volume of water vapour that would be produced from the combustion of 815.74 grams of propane (C_3H_8) with 1,006.29 grams of oxygen gas, under a pressure of 1.05 atm and a temperature of 350. degrees C.

Learn more about the ideal gas here:

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