if you could just help me set them up the would do me some good. Thanx
A. In the single reaction of chlorine and potassium bromide, how many grams of potassium chloride can be produced from 200.g each of chlorine and potassium bromide? Identify the limiting reactants.
B. In the single replacement reaction of chlorine and potassium bromide, how many of potasuim chloride are produced from 75. g of potassium bromide?
C. Calcutate the % yield for the combustion reaction of methane, CH4, whe 100. g of methane react with an excess Oxygen gas to produce water and 230.g of carbon dioxide.
D. In the single replacemt. reaction of chlorine and potassium broide, what is the % yield if 100. g of chlorine react with an excess of potassium broide to produce 310.g of bromine?
E.How many moles of lithium chloride will be formed by the reaction of chlorine with 0.046 mol of lithium bromide?
G. Cal. the percent yield in each of the following cases
a. theoreitcal yield is 50.0g of product: actual yield is 41.9g
b. theoreitcal yield is 290kg of product: actual yield is 20kg
H. Phosporus burns in air of produce phosphorus oxide. What is the mass of Phosphorus will be needed ti produce 3.25 mol of P4O10?
I. alumium will react with sulfuric aid in a single replacement reaction. How many moles of H2SO4 will reeact with 18 mol of Al
You should limit your posts to one problem (or perhaps two small ones). I will try to help you with pieces of this.
A. In the single reaction of chlorine and potassium bromide, how many grams of potassium chloride can be produced from 200.g each of chlorine and potassium bromide? Identify the limiting reactants.
1. Write the equation and balance it.
Cl2 + 2KBr ==> Br2 + 2KCl
a. Convert 200 g Cl2 to mols. # mols = g/molar mass.
b. Convert 200 g KBr to mols.
c1. Using the coefficients in the balanced equation, convert mols Cl2 to mols KCl.
c2. Using the same procedure, convert mols KBr to mols KCl.
c3. Note that either c1 or c2 is larger. The smaller of the two will be the mols KCl that will be produced and that material will be the limiting reagent.
d. Convert mols KCl produced to grams.
g = mols x molar mass.
B. In the single replacement reaction of chlorine and potassium bromide, how many of potasuim chloride are produced from 75. g of potassium bromide?
Note: how many of what are produced by 75 g KBr. U suppose you mean how many grams of KCl etc.
Follow the same procedure for the first one except that you don't know have a limiting reagent for the problem has only one reactant, not two.
Convert 75 g KBr to mols.
Convert mols KBr to mols KCl
Convert mols KCl to g KCl.
C. Calcutate the % yield for the combustion reaction of methane, CH4, whe 100. g of methane react with an excess Oxygen gas to produce water and 230.g of carbon dioxide.
Write the balanced equation.
Convert 100 g CH4 to mols.
Using the coefficients in the balanced eqution convert mols CH4 to mols CO2.
Convert mols CO2 to g CO2.
Note how these problems are woked by the same procedure.
That number of grams of CO2 is the theoretical yield of the reaction.
% yield = [amt CO2 produced/theoretical yield]*100 = [230/theoretical yield]*100 = ??
I think you get the idea how to do them. These stoichiometry problems really just follow a simple pattern. Post any follow up questions about the others but show you work. It will make it easier to know what you don't understand.
how i can convert gm to KCL
So we have a question for chem. homework and i really don't understand. can you please explain it.....
Question:There is a change in the type of oxides formed with the period three elements. Indicate the type of compounds formed (ionic, amphoteric, covalent) when the period three elements react with oxygen. Give balanced equations.
A. To determine the limiting reactant and the grams of potassium chloride produced, you will need to calculate the number of moles of chlorine and potassium bromide present in the given amounts. Then, use the balanced chemical equation to determine the stoichiometric ratio between chlorine, potassium bromide, and potassium chloride. The reactant that produces the least amount of potassium chloride is the limiting reactant.
1. Calculate the number of moles of chlorine:
moles of chlorine = mass of chlorine (in grams) / molar mass of chlorine
2. Calculate the number of moles of potassium bromide:
moles of potassium bromide = mass of potassium bromide (in grams) / molar mass of potassium bromide
3. Use the balanced chemical equation to determine the stoichiometric ratio between chlorine, potassium bromide, and potassium chloride. For example:
Cl2 + 2 KBr -> 2 KCl + Br2
The stoichiometric ratio between chlorine and potassium chloride is 1:2.
The stoichiometric ratio between potassium bromide and potassium chloride is 2:2.
4. Using the stoichiometric ratios, determine which reactant will produce the least amount of potassium chloride. The reactant that produces the least amount is the limiting reactant.
5. To determine the grams of potassium chloride produced, use the stoichiometric ratio between the limiting reactant and potassium chloride. For example, if chlorine is the limiting reactant:
moles of potassium chloride = (moles of chlorine) × 2
grams of potassium chloride = (moles of potassium chloride) × molar mass of potassium chloride
B. Similar to question A, you need to calculate the number of moles of potassium bromide from the given mass. Then, use the balanced chemical equation to determine the stoichiometric ratio between potassium bromide and potassium chloride. Convert the number of moles of potassium bromide to moles of potassium chloride using the stoichiometric ratio, and finally convert moles of potassium chloride to grams.
C. The percent yield can be calculated by dividing the actual yield by the theoretical yield and multiplying by 100.
1. Calculate the theoretical yield of carbon dioxide by determining the number of moles of methane reacted using its molar mass and stoichiometric ratio in the balanced chemical equation.
2. Calculate the percent yield using the formula:
% yield = (actual yield of carbon dioxide / theoretical yield of carbon dioxide) × 100
D. Similar to question C, calculate the theoretical yield of bromine by determining the number of moles of chlorine reacted using its molar mass and stoichiometric ratio in the balanced chemical equation. Then, calculate the percent yield using the formula.
E. To determine the moles of lithium chloride formed, first, find the stoichiometric ratio between lithium bromide and chlorine using the balanced chemical equation. The stoichiometric ratio will give you the conversion factor between moles of lithium bromide and moles of lithium chloride. Multiply the given number of moles of lithium bromide by the conversion factor to find the moles of lithium chloride.
G. For each case, divide the actual yield by the theoretical yield and multiply by 100 to calculate the percent yield.
H. Use the stoichiometric ratio between phosphorus and phosphorus oxide in the balanced chemical equation to determine the number of moles of phosphorus oxide produced. Then, calculate the molar mass of phosphorus and multiply it by the number of moles of phosphorus oxide to find the mass of phosphorus needed.
I. Determine the stoichiometric ratio between aluminum and sulfuric acid in the balanced chemical equation. Multiply the given number of moles of aluminum by the stoichiometric ratio to find the number of moles of sulfuric acid that will react.