In The Reaction M G C L 2 + 2 K O H → M G ( O H ) 2 + 2 K C L MgCl_2 + 2 KOH \rightarrow Mg(OH)_2 + 2 KCl M G C L 2 ​ + 2 K O H → M G ( O H ) 2 ​ + 2 K Cl , How Many Grams Of KOH React With 1 Mole Of M G C L 2 MgCl_2 M G C L 2 ​ ?A. 95 G B. ( 2 ) ( 56 G (2)(56 \text{ G} ( 2 ) ( 56 G ] C. 56 G D. ( 1 2 ) ( 56 G \left(\frac{1}{2}\right)(56 \text{ G} ( 2 1 ​ ) ( 56 G ]

Understanding the Chemical Reaction

The given chemical reaction is $MgCl_2 + 2 KOH \rightarrow Mg(OH)_2 + 2 KCl$. This reaction involves the reaction of magnesium chloride ($MgCl_2$) with potassium hydroxide (KOH) to form magnesium hydroxide ($Mg(OH)_2$) and potassium chloride (KCl).

Balancing the Chemical Equation

To balance the chemical equation, we need to ensure that the number of atoms of each element is the same on both the reactant and product sides. In this case, the balanced equation is already given, but let's break it down:

• Magnesium (Mg) is present in equal amounts on both sides (1 mole).
• Chlorine (Cl) is also present in equal amounts on both sides (2 moles).
• Potassium (K) is present in equal amounts on both sides (2 moles).
• Hydroxide (OH) is present in equal amounts on both sides (2 moles).

Stoichiometry and Molar Ratios

Now that we have a balanced chemical equation, we can use stoichiometry to determine the number of moles of KOH required to react with 1 mole of $MgCl_2$. According to the balanced equation, 2 moles of KOH are required to react with 1 mole of $MgCl_2$. This is a 1:2 molar ratio.

Calculating the Mass of KOH

To calculate the mass of KOH required to react with 1 mole of $MgCl_2$, we need to know the molar mass of KOH. The molar mass of KOH is 56 g/mol (potassium = 39 g/mol, oxygen = 16 g/mol, and hydrogen = 1 g/mol).

Since we need 2 moles of KOH to react with 1 mole of $MgCl_2$, we can calculate the mass of KOH required as follows:

Mass of KOH = (2 moles) x (56 g/mol) = 112 g

However, this is not an option in the given choices. Let's re-examine the choices:

A. 95 g B. (2)(56 g) C. 56 g D. (1/2)(56 g)

Choosing the Correct Answer

Based on our calculation, the correct answer is:

B. (2)(56 g)

This is because we need 2 moles of KOH to react with 1 mole of $MgCl_2$, and each mole of KOH has a mass of 56 g. Therefore, the total mass of KOH required is 2 x 56 g = 112 g.

However, this is not the answer choice. Let's re-examine the calculation:

We need 2 moles of KOH to react with 1 mole of $MgCl_2$, and each mole of KOH has a mass of 56 g. Therefore, the total mass of KOH required is indeed 2 x 56 g = 112 g.

However, the answer choice is (2)(56 g), which is equivalent to 112 g. Therefore, the correct answer is indeed B. (2)(56 g).

Conclusion

In conclusion, to determine the number of grams of KOH required to react with 1 mole of $MgCl_2$, we need to use stoichiometry and the molar mass of KOH. The correct answer is B. (2)(56 g), which is equivalent to 112 g.

Additional Tips and Tricks

• Always balance the chemical equation before using stoichiometry.
• Use the molar mass of each substance to calculate the mass required.
• Make sure to use the correct molar ratio from the balanced equation.
• Double-check your calculations to ensure accuracy.

Common Mistakes to Avoid

• Failing to balance the chemical equation.
• Using the wrong molar ratio from the balanced equation.
• Not using the correct molar mass of each substance.
• Not double-checking calculations for accuracy.

Real-World Applications

• Stoichiometry is used in a wide range of applications, including chemistry, biology, and engineering.
• Understanding stoichiometry is crucial for designing and optimizing chemical reactions.
• Stoichiometry is used in the production of chemicals, pharmaceuticals, and other materials.

Final Thoughts

In conclusion, stoichiometry is a powerful tool for determining the amount of reactants required to produce a specific amount of product. By balancing the chemical equation and using the molar mass of each substance, we can calculate the mass of KOH required to react with 1 mole of $MgCl_2$. Remember to always balance the chemical equation, use the correct molar ratio, and double-check your calculations for accuracy.

Q: What is the difference between a balanced chemical equation and an unbalanced equation?

A: A balanced chemical equation has the same number of atoms of each element on both the reactant and product sides. An unbalanced equation does not have the same number of atoms of each element on both sides.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to ensure that the number of atoms of each element is the same on both the reactant and product sides. You can do this by adding coefficients (numbers in front of the formulas of the reactants or products) to balance the equation.

Q: What is stoichiometry?

A: Stoichiometry is the study of the quantitative relationships between reactants and products in chemical reactions. It involves using the molar masses of substances to calculate the amount of reactants required to produce a specific amount of product.

Q: How do I use stoichiometry to calculate the mass of a substance?

A: To use stoichiometry to calculate the mass of a substance, you need to know the molar mass of the substance and the number of moles required to produce a specific amount of product. You can then use the formula: mass = moles x molar mass.

Q: What is the molar mass of a substance?

A: The molar mass of a substance is the mass of one mole of the substance. It is calculated by adding the atomic masses of all the atoms in the substance.

Q: How do I calculate the molar mass of a substance?

A: To calculate the molar mass of a substance, you need to know the atomic masses of all the atoms in the substance. You can then add these atomic masses together to get the molar mass.

Q: What is the difference between a mole and a gram?

A: A mole is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules). A gram is a unit of mass that represents 1/1000 of a kilogram.

Q: How do I convert between moles and grams?

A: To convert between moles and grams, you can use the formula: moles = mass / molar mass.

Q: What is the significance of stoichiometry in real-world applications?

A: Stoichiometry is used in a wide range of applications, including chemistry, biology, and engineering. It is used to design and optimize chemical reactions, to calculate the amount of reactants required to produce a specific amount of product, and to predict the yield of a reaction.

Q: What are some common mistakes to avoid when using stoichiometry?

A: Some common mistakes to avoid when using stoichiometry include:

• Failing to balance the chemical equation
• Using the wrong molar ratio from the balanced equation
• Not using the correct molar mass of each substance
• Not double-checking calculations for accuracy

Q: How can I practice using stoichiometry?

A: You can practice using stoichiometry by working through problems and exercises that involve calculating the mass of a substance or the amount of reactants required to produce a specific amount of product. You can also use online resources and calculators to help you practice.

Q: What are some resources available for learning more about stoichiometry?

A: Some resources available for learning more about stoichiometry include:

• Online tutorials and videos
• Textbooks and study guides
• Online calculators and software
• Practice problems and exercises
• Online communities and forums

Q: How can I apply stoichiometry to real-world problems?

A: You can apply stoichiometry to real-world problems by using it to design and optimize chemical reactions, to calculate the amount of reactants required to produce a specific amount of product, and to predict the yield of a reaction. You can also use stoichiometry to solve problems in fields such as chemistry, biology, and engineering.