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Ilia_Sergeevich [38]
3 years ago
6

Heating oxygen difluoride gas yields oxygen gas and fluorine gas? Whats the balance chemical equation for this?

Chemistry
1 answer:
N76 [4]3 years ago
5 0
2OF2(g) —> O2(g) + 2F2(g) hope that helps
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Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300 °C, [
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Answer:

rate=-1.75x10^{-5}\frac{M}{s}

Explanation:

Hello,

In this case, for the given information, we can compute the rate of disappearance of NO₂ by using the following rate relationship:

rate=\frac{1}{2}*\frac{C_f-C_0}{t_f-t_0}

Whereas it is multiplied by the the inverse of the stoichiometric coefficient of NO₂ in the reaction that is 2. Moreover, the subscript <em>f</em> is referred to the final condition and the subscript <em>0</em> to the initial condition, thus, we obtain:

rate=\frac{1}{2}*\frac{0.00650M-0.0100M}{100s-0s}\\\\rate=-1.75x10^{-5}\frac{M}{s}

Clearly, it turns out negative since the concentration is diminishing due to its consumption.

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A student dissolves of styrene in of a solvent with a density of . The student notices that the volume of the solvent does not c
raketka [301]

Answer:

0.576M and 0.655m

Explanation:

<em>...Dissolves 15.0g of styrene (C₈H₈) in 250.mL of a solvent with a density of 0.88g/mL...</em>

<em />

Molarity is defined as moles of solute (Styrene in this case) per liter of solution whereas molality is the moles of solute per kg of solvent. Thus, we need to find the moles of styrene, the volume in liters of the solution and the mass in kg of the solvent as follows:

<em>Moles styrene:</em>

Molar mass C₈H₈:

8C = 12.01g/mol*8 = 96.08g/mol

8H = 1.005g/mol* 8 = 8.04g/mol

96.08g/mol + 8.04g/mol = 104.12g/mol

Moles of 15.0g of styrene are:

15.0g * (1mol / 104.12g) = 0.144 moles of styrene

<em>Liters solution:</em>

250mL * (1L / 1000mL) = 0.250L

<em>kg solvent:</em>

250mL * (0.88g/mL) * (1kg / 1000g) = 0.220kg

Molarity is:

0.144 moles / 0.250L =

<h3>0.576M</h3>

Molality is:

0.144 moles / 0.220kg =

<h3>0.655m</h3>
8 0
3 years ago
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