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3 years ago

Compare magnesium oxide and carbon dioxide

1 answer:

4 0

Answer:Magnesium is higher in the reactivity series than carbon so it is more reactive than carbon and removes the oxygen from the carbon dioxide (to give carbon and magnesium oxide).

Explanation:

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Acetylene (C2H2) gas is often used in welding torches because of the very high heat produced when it reacts with oxygen (O2) gas

babymother [125]

Answer:

0.05 mol

Explanation:

The balanced equation for the reaction that takes place is:

2C₂H₂ (g) + 5O₂ (g) → 4CO₂ (g) + 2H₂O (g)

Now we<u> convert 0.10 moles of carbon dioxide (CO₂) into moles of acetylene (C₂H₂)</u>, using the <em>stoichiometric coefficients of the balanced reaction</em>:

0.10 mol CO₂ * $\frac{2molC_2H_2}{4molCO_2}$ = 0.05 mol C₂H₂

7 0

3 years ago

Ammonia is formed according to the reaction below. A chemist mixes 21 grams of nitrogen gas and 18 grams of hydrogen gas in a 2.

Rama09 [41]

Answer : The mass of hydrogen gas consumed will be, 4.5 grams

Explanation : Given,

Mass of $N_2$ = 21 g

Mass of $H_2$ = 18 g

Molar mass of $N_2$ = 28 g/mole

Molar mass of $H_2$ = 2 g/mole

First we have to calculate the moles of $N_2$ and $H_2$ .

$\text{Moles of }N_2=\frac{\text{Mass of }N_2}{\text{Molar mass of }N_2}=\frac{21g}{28g/mole}=0.75moles$

$\text{Moles of }H_2=\frac{\text{Mass of }H_2}{\text{Molar mass of }H_2}=\frac{18g}{2g/mole}=9moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$

From the given balanced reaction, we conclude that

As, 1 mole of $N_2$ react with 3 moles of $H_2$

So, 0.75 moles of $N_2$ react with $3\times 0.75=2.25$ moles of $H_2$

From this we conclude that, $H_2$ is an excess reagent because the given moles are greater than the required moles and $N_2$ is a limiting reagent because it limits the formation of product.

The moles of hydrogen gas consumed = 2.25 mole

Now we have to calculate the mass of hydrogen gas consumed.

$\text{Mass of }H_2=\text{Moles of }H_2\times \text{Molar mass of }H_2$

$\text{Mass of }H_2=(2.25mole)\times (2g/mole)=4.5g$

Therefore, the mass of hydrogen gas consumed will be, 4.5 grams

5 0

4 years ago

D. 100 mph

Andrej [43]

Answer:

The answer is c

Explanation:

200 divided by 100 is 2 and you can check that by multiplying 2 by 100.

4 0

3 years ago

How much heat is required to raise the temperature of 25.0 grams of waterfrom 75.0°C to its boiling point?

Sav [38]

Answer:

How much heat is required to raise the temperature of 25.0 grams of waterfrom 75.0°C to its boiling point?

Explanation:

5 0

3 years ago

Hydrochloric acid reacts with sodium hydroxide to produce sodium chloride and water. If 20.6 g of sodium hydroxide reacts with a

astraxan [27]

Answer:

30.1 g NaCl

Explanation:

Your first conversion is converting grams NaOH to moles of NaOH using its molar mass (39.997 g/mol). Then, use the mole ratio of 1 mol NaCl for every 1 mol NaOH to get to moles of NaCl. Then finally multiply by the molar mass of NaCl (58.44 g/mol) to get grams of NaCl.

20.6 g NaOH • (1 mol NaOH / 39.997 g NaOH) • (1 mol NaCl / 1 mol NaOH) • (58.44 g NaCl / 1 mol NaCl) = 30.1 g NaCl

4 0

3 years ago