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3 years ago

1. Is the reaction between magnesium and oxygen in the air spontaneous?

Chemistry

1 answer:

Vikki [24]3 years ago

4 0

Answer:

Once ignited, a ribbon of magnesium metal burns freely in air to form solid magnesium oxide in the form of a white powder. The reaction is plainly spontaneous even though ΔS is negative.

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The molecular weight of acetic acid is

kolezko [41]

Answer:

60.052 grams per mole

8 0

3 years ago

A flexible container at an initial volume of 6.13 L contains 2.51 mol of gas. More gas is then added to the container until it r

aleksley [76]

Answer:

2.12 moles of gas were added.

Explanation:

We can solve this problem by using Avogadro's law, which states that at constant temperature and pressure:

V₁n₂=V₂n₁

Where in this case:

V₁ = 6.13 L

n₂ = ?

V₂ = 11.3 L

n₁ = 2.51 mol

We input the data:

6.13 L * n₂ = 11.3 L * 2.51 mol

n₂ = 4.63

As 4.63 moles is the final number of moles, the number of moles added is:

4.63 - 2.51 = 2.12 moles

5 0

2 years ago

112 g of aluminum carbide react with 174 g water to produce methane and aluminum hydroxide in the reaction shown below.

dolphi86 [110]

Answer: 4.999 moles of excess reactant will be left over.

Explanation:

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of aluminium carbide = 112 g

Molar mass of aluminium carbide = 143.96 g/mol

Putting values in equation 1:

$\text{Moles of aluminium carbide}=\frac{112g}{143.96g/mol}=0.778mol$

For the given chemical reaction:

$2Al_4C_3(s)+12H_2O(l)\rightarrow 3CH_4(g)+4Al(OH)_3(s)$

By the stoichiometry of the reaction:

2 moles of aluminium carbide reacts with 12 moles of water

So, 0.778 moles of aluminium carbide will react with = $\frac{12}{2}\times 0.778=4.668 mol$ of water

Given mass of water = 174 g

Molar mass of water = 18 g/mol

Putting values in equation 1:

$\text{Moles of water}=\frac{174g}{18g/mol}=9.667mol$

Moles of excess reactant (water) left = 9.667 - 4.668 = 4.999 moles

Hence, 4.999 moles of excess reactant will be left over.

8 0

2 years ago

If an element has a mass number of 222 and an atomic number of 86, how

svlad2 [7]

Answer:

136

Explanation:

The Mass Number is the combination of the amount of Protons and Neutrons in an element, so if the total mass is 222, and the amount of protons is 86, then you can do 86 + x = 222 to find that x is equal to 136

5 0

3 years ago

Do atoms lend and borrow electrons from inner shells

zaharov [31]

False. They don't borrow electrons at all. They already have their respective electron affinities. This is called as electronegativity, and it's an occurence where it already has its own from its actual structure. It never borrows any electrons at all.

4 0

3 years ago

1. Is the reaction between magnesium and oxygen in the air spontaneous?​

1. Is the reaction between magnesium and oxygen in the air spontaneous?