Chemistry

posted by .

In a reaction chamber, 3.0mol of aluminum is mixed with 5.3mol Cl2 and reacts. The reaction is described by the following balanced chemical equation.

2Al + 3Cl2 ==> 2AlCl3

a)Identify the limiting reagent for the reaction.
b)Calculate the number of moles or products formed
c)Calculate the number of moles of excess reagent remaining after the reaction.

• Chemistry -

Most limiting reagent problems are worked the same way. Print these instructions and memorize them.
1. Write and balanced the equation. You have that.

2. USUALLY you are given grams and you must convert to moles by moles = grams/molar mass. This already has the moles given and you can skip this step.

3a. Using the coefficients in the balanced equation, convert 3.0 moles Al to moles of AlCl3.
3b. Same procedure but convert 5.3 moles Cl2 to moles AlCl3.
3c. It is quite likely that the answer to 3a and 3b will not be the same which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent.

4. USUALLY, the problem asks for grams here and you would calculate grams AlCl3 from the smaller value = moles x molar mass. That isn't needed here since they don't ask for it but this is useful information for the future.

5. To do part d, you have identified the limiting reagent. The other reagent is not limiting; therefore, there will be some that remains unreacted. To know the final value, use the coefficients (as in step 3 above) to determine the moles that react with ALL of the limiting reagent, subtract from the initial amount, the different is the amount remaining unreacted. If you wish (although the problem doesn't ask for it), you can multiply moles remaining x molar mass to arrive at the grams of the other reactant after the reaction.

• Chemistry -

Ss

Similar Questions

1. CHEM

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3Cl2(g) -> 2AlCl3(s) You are given 19.0g of aluminum and 24.0g of chlorine gas. a)If you had excess chlorine, how many moles of of …
2. CHEM-last part prob.

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3Cl2(g) -> 2AlCl3(s) You are given 19.0g of aluminum and 24.0g of chlorine gas. a)If you had excess chlorine, how many moles of of …
3. Chemistry

Aluminum cookware is reffered ti as "anodized aluminum". The anodizing process puts a layer of aluminum oxide on the aluminum, protecting it from corrosion. Consider the reaction of 10.00 grams of aluminum with 10.00 grams of oxygen …
4. Chemistry

How much heat (in kilojoules) is released on reaction of 4.10 g of Al?
5. Chemistry

4. Write the balanced equation for CH4+Cl2„_CH2Cl2+HCl 4a. For the reaction in problem 4, ƒ´H = -118.3 kcal/mol. Identify whether this is an exothermic or endothermic reaction. Calculate the ƒ´H when 6.00 g of Cl2 are used in …
6. College Chem

4. Write the balanced equation for CH4+Cl2„_CH2Cl2+HCl6. For the reaction in problem 4, Heat of Reaction = -118.3 kcal/mol. Identify whether this is an exothermic or endothermic reaction. Calculate the Heat of Reaction when 6.00 …
7. Chemistry

Hi, I posted my question earlier but I was having some difficulty with it. 2Al+ 3Cl2-->2AlCl3 You are given 31.0g of aluminum and 36.0g of chlorine gas. 1.If you had excess chlorine, how many moles of aluminum chloride could be …
8. CHEMISTRY

1. Consider the following reaction: Pb(NO3)2+KI--> Pbl2 +KNO3 in theis experiment, 12.0g of Kl is reacted with 20.5g of Pb(NO3)2. a) write a balanced equation for this reaction. b)identify the limiting reaction. c)calculate the …
9. Chemistry

can you please please help me with these questions I don't know how to do any of them. I know how to calculate moles and grams and mole ratio,etc but I don't understand the limiting excess reactant and yield stuff. Thanks! 1.In the …
10. Chemistry

can you please please help me with these questions I don't know how to do any of them. I know how to calculate moles and grams and mole ratio,etc but I don't understand the limiting excess reactant and yield stuff. Thanks! 1.In the …

More Similar Questions

Post a New Question