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1 year ago

The molar mass of an imaginary molecule is is 93.89 g/mol. Determine its density at STP.

Chemistry

1 answer:

Igoryamba1 year ago

3 0

Answer:

Density = 4.191 gm/L

Explanation:

Given:

Molar mass = 93.89 g/mol

Volume(Missing) = 22.4 L (Approx)

Find:

Density at STP

Computation:

Density = Mass/Volume

Density = 93.89 / 22.4

Density = 4.191 gm/L

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Answer:

The intermolecular bonding in the solid is van der Waals dispersion forces. That means that it will have a lower melting point than diamond or graphite where you have giant covalent bonding. In fact C60 sublimes at 800 K (527°C). Diamond and graphite sublime at around 4000 K.

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Consider the reaction. 2c(s,graphite) h2= c2h2(g) Based on the equation and the information in the table, what is the enthalpy o

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<h3>The enthalpy of the reaction : C.226.73 kJ</h3><h3>Further explanation</h3>

Delta H reaction (ΔH) is the amount of heat change between the system and its environment

(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)

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Delta H reaction (ΔH) is the difference between product enthalpy and reactant enthalpy (Hp-Hr)

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From the available data: Hf (kJ / mol) C2 H2 (g)= 226.73

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<h3>Learn more</h3>

(ΔH) reaction

brainly.com/question/1889660

Keywords : (ΔH) reaction, C2H2

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E = $Q \times V$

Hence, putting the given values into the above formula and then calculate the value of electricity as follows.

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Hence, $\frac{9.4 \times 10^{7}}{2.77 \times 10^{-7}}$ kWh

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