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nevsk [136]
8 months ago
8

When menthol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it

is often used as a fuel in high performance racing cars. The combination of methanol has the balanced, thermochemical equation CH3OH(g) + 3/2O2(g) — CO2(g) + 2H2O(1) DeltaH= -764Kj How much methanol, in grams, must be found to produce 701 kj of heat?
Chemistry
1 answer:
Drupady [299]8 months ago
5 0

We have the following balanced equation:

CH_3OH_{(g)}+\frac{3}{2}O_{2\text{ (g)}}\rightarrow CO_{2\text{ (g)}}+2H_2O_{(l)}

They also give us the heat of reaction equal to -764 kJ, i.e. it is an exothermic reaction.

By observing the reaction, we can deduce that for this heat to be generated, one mole of methanol is needed. Now let's see how many grams that mole of methanol equals. We will use the molecular weight equal to 32.04 g/mol

\begin{gathered} g\text{ of methanol = 1 mol }\times\text{ 32.04 g/mol} \\ g\text{ of methanol }=\text{ 32.04 g} \end{gathered}

Now we know the grams of methanol that generate 764 kJ, because the heat of reaction is directly proportional to the mass of the reactants, we can apply a rule of three to know the grams needed to produce a heat of reaction equal to 701 kJ:

\begin{gathered} \frac{32.04\text{ g of methanol}}{764\text{ kJ}}=\text{ }\frac{x\text{ g of methanol}}{701\text{ kJ}} \\ x\text{ g of methanol = }\frac{32.04\text{ g of methanol }\times\text{ 701 kJ}}{764\text{ kJ}} \\ g\text{ of methanol = 29.4 g} \end{gathered}

So, 29.4 g of methanol must be found to produce 701 kJ of heat

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taurus [48]

Answer:

The balanced chemical equation is given as:

2Mg(s)+O_2(g)\rightarrow 2MgO(s)

Explanation:

When magnesium metal burns in presence of oxygen it gives white color powdered compound called magnesium oxide.

The balanced chemical equation is given as:

2Mg(s)+O_2(g)\rightarrow 2MgO(s)

According to reaction, 2 moles of magnesium metal when reacts with 1 mole of oxygen gas it gives 2 moles of  solid magnesium oxide.

3 0
2 years ago
When the electron of a hydrogen atom moves into a higher energy orbit, what is the state of the atom?
faltersainse [42]
Answer is: <span>excited state.
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4 0
2 years ago
Compound X has a molar mass of 416.48 g mol
bazaltina [42]

Answer:

P₂Cl₁₀

Explanation:

From the question given above, the following data were obtained:

Molar mass of compound X = 416.48 g/mol

Percentage of phosphorus (P) = 14.87%

Percentage of Chlorine (Cl) = 85.13%

Molecular formula of X =?

Next, we shall determine the empirical formula of compound X. This can be obtained as follow:

P = 14.87%

Cl = 85.13%

Divide by their molar mass

P = 14.87 / 31 = 0.480

Cl = 85.13 / 35.5 = 2.398

Divide by the smallest

P = 0.480 / 0.480 = 1

Cl = 2.398 / 0.480 = 5

Empirical formula of compound X is PCl₅

Finally, we shall determine the molecular formula of compound X. This can be obtained as follow:

Molar mass of compound X = 416.48 g/mol

Empirical formula = PCl₅

Molecular formula =?

Molecular formula= [Empirical formula]ₙ

[PCl₅]ₙ = 416.48

[31 + (35.5 × 5)]ₙ = 416.48

[31 + 177.5]n = 416.48

208.5n = 416.48

Divide both side by 208.5

n = 416.48 / 208.5

n = 2

Molecular formula = [PCl₅]ₙ

Molecular formula = [PCl₅]₂

Molecular formula = P₂Cl₁₀

Therefore, the molecular formula of compound X is P₂Cl₁₀

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