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2 years ago

Zinc Sulfide reacts with oxygen according to the reaction:

Chemistry

1 answer:

zhuklara [117]2 years ago

6 0

The amount in moles of the excess reactant left is 0.5 mole

<h3>Balanced equation</h3>

2ZnS (s) + 3O₂(g) --> 2ZnO (s) + 2SO₂(g)

From the balanced equation,

2 moles of ZnS reacted with 3 moles of O₂

<h3>How to determine the excess reactant</h3>

From the balanced equation,

2 moles of ZnS reacted with 3 moles of O₂

Therefore,

4.2 moles of ZnS will react with =(4.2 × 3) / 2 = 6.3 moles of O₂

From the calculations made above, we can see that only 6.3 moles of O₂ out of 6.8 moles given, is required to react completely with 4.2 moles of ZnS.

Thus, ZnS is the limiting reactant and O₂ is the excess reactant.

<h3> How to determine the mole of the excess reactant remaining</h3>

The excess reactant is O₂. Thus the mole remaining after the reaction can be obtained as illustrated below:

Mole of O₂ given = 6.8 moles
Mole of O₂ that reacted = 6.3 moles
Mole of O₂ remaining =?

Mole of O₂ remaining = (Mole of O₂ given) - (Mole of O₂ that reacted)

Mole of O₂ remaining = 6.8 - 6.3

Mole of O₂ remaining = 0.5 mole

Learn more about stoichiometry:

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What is the percent composition of hydrogen in glucose

Ulleksa [173]

Answer:

Explanation:

<h2>Thus the % composition of glucose by mass is carbon 40.0 % oxygen 53.3 % hydrogen 6.7 % in this way, the % composition by mass of any compound can be calculated provided that is formed is known. </h2>

6 0

3 years ago

What molarity is prepared when a solution contains 0.277 moles of calcium bromide in 500 mL of solution (must change mL to Liter

Vladimir79 [104]

Answer:

0.554M of Calcium Bromide

Explanation:

Molarity by defintion is #of moles of something/litres of solution.

Therefore, here, we have 0.277 moles of calcium bromide and 500mL (divide 500ml by 1000 to go from mL to L because for every 1L there's 1000mL) or 0.5L.

Molarity= 0.277/0.5 = 0.554M of Calcium Bromide

5 0

3 years ago

How many liters of carbon dioxide will 0.5 moles of lithium hydroxide (LiOH) absorb?

Elden [556K]

Answer : The volume of carbon dioxide will be, 5.6122 L

Solution : Given,

Moles of LiOH = 0.5 moles

Molar mass of carbon dioxide = 44 g/mole

Density of carbon dioxide = 0.00196 g/ml

First we have to calculate the mass of carbon dioxide.

The balanced reaction will be,

$2LiOH+CO_2\rightarrow Li_2CO_3+H_2O$

From the reaction we conclude that

As, 2 moles of LiOH absorbs 44 grams of carbon dioxide

So, 0.5 moles of LiOH absorbs $\frac{0.5moles}{2moles}\times 44g=11$ grams of carbon dioxide

Mass of carbon dioxide = 11 g

Density of carbon dioxide = 0.00196 g/ml

Now we have to calculate the volume of carbon dioxide.

$Density=\frac{Mass}{volume}$

$0.00196g/ml=\frac{11g}{volume}$

Volume of carbon dioxide = 5612.24 ml = 5.6122 L (1 L = 1000 ml)

Therefore, the volume of carbon dioxide will be, 5.6122 L

5 0

3 years ago

Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction betwe

shusha [124]

Answer: The reaction order with respect to A is m

Explanation:

Order of the reaction is defined as the sum of the concentration of terms on which the rate of the reaction actually depends. It is the sum of the exponents of the molar concentration in the rate law expression.

Elementary reactions are defined as the reactions for which the order of the reaction is same as its molecularity and order with respect to each reactant is equal to its stoichiometric coefficient as represented in the balanced chemical reaction.

For the given reaction:

$aA+bB\rightleftharpoons cC+dD$

$Rate=k[A]^m[B]^n$

In this equation, the order with respect to each reactant is not equal to its stoichiometric coefficient which is represented in the balanced chemical reaction.

Hence, this is not considered as an elementary reaction.

Order with respect to A = m

Order with respect to B = n

Overall order = m+n

Thus order with respect to A is m.

3 0

3 years ago

In experiment 1, how many moles of benzoic acid are present? how many moles of sodium bicarbonate are contained in 1 ml of a 10%

nexus9112 [7]

First, let us calculate the moles of solute or sodium bicarbonate is in the 1 ml solution.

<span>moles = 1 mL * (1 g / 9 mL) = 0.11 moles</span>

The molar mass of sodium bicarbonate is 84 g/mol, therefore the mass is:

mass = 0.11 moles * 84 g/mol

6 0

3 years ago