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Stella [2.4K]
3 years ago
11

How many moles are in a sample of 4.55 x 10^24 molecules of C3H8?​

Chemistry
1 answer:
mestny [16]3 years ago
7 0

Answer: 7.56 moles

Explanation:

C3H8 is the chemical formula for propane, the third member of the alkane family.

Recall that based on Avogadro's number, 1 mole of any substance has 6.02 x 10^23 atoms

So 1 mole of C3H8 = 6.02 x 10^23 atoms

Z moles of C3H8 = 4.55 x 10^24 atoms

To get the value of Z, we cross multiply:

1 x 4.55 x 10^24 atoms = Z moles x (6.02 x 10^23 atoms)

4.55 x 10^24 atoms = Z moles x (6.02 x 10^23 atoms)

To get the value of Z divide both sides by 6.02 x 10^23 atoms

Z moles =4.55 x 10^24 atoms ➗ 6.02 x 10*23 atoms

Hence, Z = 7.56 moles

Thus, the number of propane, C3H8 is 7.56 moles

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the ideal gas law is PV = nRT, so in the terms of n,

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n = (700 * 2) / (8.31 * 450)

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Calculate the amount of heat that must be absorbed by 10.0 g of ice at –20°C to convert it to liquid water at 60.0°C. Given: spe
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The amount of heat to absorb is 6,261 J

Explanation:

Calorimetry is in charge of measuring the amount of heat generated or lost in certain physical or chemical processes.

The total energy required is the sum of the energy to heat the ice from -20 ° C to ice of 0 ° C, melting the ice of 0 ° C in 0 ° C water and finally heating the water to 60 ° C.

So:

  • Heat required to raise the temperature of ice from -20 °C to 0 °C

Being the sensible heat of a body the amount of heat received or transferred by a body when it undergoes a temperature variation (Δt) without there being a change of physical state (solid, liquid or gaseous), the expression is used:

Q = c * m * ΔT

Where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation (ΔT=Tfinal - Tinitial).

In this case, m= 10 g, specific heat of the ice= 2.1 \frac{J}{g*C} and ΔT=0 C - (-20 C)= 20 C

Replacing: Q= 10 g*2.1 \frac{J}{g*C} *20 C and solving: Q=420 J

  • Heat required to convert 0 °C ice to 0 °C water

The heat Q necessary to melt a substance depends on its mass m and on the called latent heat of fusion of each substance:

Q= m* ΔHfusion

In this case, being 1 mol of water= 18 grams: Q= 10 g*6.0 \frac{kJ}{mol} *\frac{1 mol of water}{18 g}= 3.333 kJ= 3,333 J (being kJ=1,000 J)

  • Heat required to raise the temperature of water from 0 °C to 60 °C

In this case the expression used in the first step is used, but being: m= 10 g, specific heat of the water= 4.18 \frac{J}{g*C} and ΔT=60 C - (0 C)= 60 C

Replacing: Q= 10 g*4.18 \frac{J}{g*C} *60 C and solving: Q=2,508 J

Finally, Qtotal= 420 J + 3,333 J + 2,508 J

Qtotal= 6,261 J

<u><em> The amount of heat to absorb is 6,261 J</em></u>

<u><em></em></u>

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