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Mice21 [21]
3 years ago
13

Step by step on how to find limiting reactant, with an example please!

Chemistry
1 answer:
olga2289 [7]3 years ago
4 0

In order to find a limiting reactant, you'll at least need the mass of both reactants, or even better, number of moles of it (but you can work this out with the mass).

1. Write a balanced equation for the reaction. Balancing the equation is especially important because the mole ratio (the numbers when balancing) can affect the answer.

2. Find the number of moles of each reactant. You can find this by dividing the mass in grams by the molar mass of substance (adding all atomic masses of all elements present).

3.  Find the actual number of moles needed in the reaction by considering the mole ratio from the equation. Which means, if the mole ratio of reactant A : reactant B is 1:1, you don't need to change anything, but, if its somewhat 2:1 or 2:3 etc, you have to multiply or divide the n.o.m.s to make the mole ratio balanced. (You can refer to example if this part is a bit confusing)

4.  Determine which reactant has the least number of moles. That one is the limiting reactant!

Example (Question took from 2013 IGCSE Chemistry Paper3);

"4.8g of calcium is added to 3.6 g of water. The following reaction occurs.

Ca + 2H2O → Ca(OH)2 + H2

Find the limiting reactant."

1. The balanced equation is already given, so you're good for this step!

2. Find the n.o.m.s for the 2 reactants.

no. of moles of Ca

= 4.8 / 40.1

= 0.1197 mol

no. of moles of H2O

= 3.6 / (1.0 x 2 + 16.0)

= 0.2 mol

3. Consider the equation again,

From equation, mole ratio of Ca:H2O = 1:2

So, no. of moles of moles of Ca = 0.1197 x 2

= 0.2394 mol

4. Since 0.2 mol is less than 0.2394mol, H2O is the limiting reactant.

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Reactioneaza total 22 kg calcar de puritate 80 % cu o solutie de acid clorhidric de concentratie 30 %. Stiind ca rezulta clorura
WINSTONCH [101]

Answer:

De la Alex;)(da alex ăla de e din cls cu tn:)

7 0
3 years ago
The work done to compress a gas is 83.0 J. As a result, 27.0 J of heat is given off to the surroundings. Calculate the change in
stellarik [79]

Answer:

ΔU° = 56.0 J

Explanation:

Step 1: Given data

  • Work done to compress the gas (w): 83.0 J (When work is done on the gas, w is positive).
  • Heat given off to the surroundings (q): -27.0 J (When heat is released to the surroundings, q is negative)

Step 2: Calculate the change in the internal energy of the gas (ΔU°)

The internal energy of a gas is the energy contained within it. We can calculate it using the following expression.

ΔU° = q + w

ΔU° = -27.0 J + 83.0 J

ΔU° = 56.0 J

5 0
3 years ago
How many molecules are there in 122 grams of Cu(NO3)2?
ipn [44]
Cu =63.5
2 times N =28.02
6 times O =96
96=63.5=28.02=127.07
122/127.07=.96 molecules
6 0
3 years ago
BRAINLIESTTT ASAP!! PLEASE HELP ME :)
Ratling [72]

Jot down the formula of the ionic compound. Let's say the ionic compound you're working with is NaCl.  

Write the name of the metal.

Add the name of the non-metal with an –ide ending.

Combine the cation and anion names.

Practice naming more simple ionic compounds.

7 0
3 years ago
Calculate the molecular (formula) mass of each compound: (a) iron(ll) acetate tetrahydrate; (b) sulfur tetrachloride; (c) potass
Nutka1998 [239]

Answer:

a) Iron(ll) acetate tetrahydrate: 245,68 g/mol

b) Sulfur tetrachloride: 173,87 g/mol

c) Potassium ermanganate 158,034 g/mol

Explanation:

To solve this kind of exercises you must look for the number of atoms in each molecule first, then look on the periodic table the atom weight and the multiply the atom weight times the quantity of each atom. For instance:

The molecule of Iron(II) acetate itetrahydrate is (CH3COO)2Fe•4H2O, it means that you have:

2 atoms of carbon times the atomic weight of C (12.00g/mol)= 24g

14 atoms of Hidrogen times the atomic weight of H (1,00g/mol)= 14g

6 atoms of Oxigen times the atomic weight of O (16,0g/mol)= 96

2 atoms of Iron times the atomic weight of Fe (55,84g/mol)= 111,68g

At last, you only have to add the results: 24+14+96+11,68= 245,68g/mol. This example was for the first molecule.

See you,

5 0
3 years ago
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