Of 1.00g of A reacts with 1.50g of B, what is the mass of C
how do i do this? Law of conservationn of mass, but not sure where to start?
...........A + B ==> C
I........1.00..1.50...0
C.......-1.00.-1.50..2.50
E.........0.....0....2.50
When chemistry fails turn to apples (A) and oranges (B). If you have 4 lbs apples in a basket and 4 lbs oranges in the same basket, you have 8 lbs of C(total mass of fruit).
To determine the mass of C, you need to determine the limiting reactant between A and B. The limiting reactant is the one that is completely consumed and determines the maximum amount of product that can be formed. Here's how you can follow this step by step:
Step 1: Calculate the number of moles of A and B.
To calculate the number of moles of a substance, divide its mass by its molar mass. The molar mass of a substance is the sum of the atomic masses of all the elements in its formula.
Given:
Mass of A = 1.00 g
Mass of B = 1.50 g
You need to know the molar masses of A and B to proceed further with the calculation.
Step 2: Determine the stoichiometric ratio between A and C and between B and C.
The stoichiometric ratio can be obtained from the balanced chemical equation for the reaction between A and B to form C.
For example, let's assume the balanced chemical equation is:
A + B → C
From this equation, you can see that the ratio between A and C is 1:1, and the ratio between B and C is also 1:1.
Step 3: Compare the moles of A and B to determine the limiting reactant.
If the stoichiometric ratio is not 1:1, you need to adjust the moles of A and B based on their respective stoichiometric ratios.
For example, let's say the stoichiometric ratio between A and C is 1:2. Then, you would double the moles of A obtained in step 1.
Compare the adjusted moles of A and B. The reactant with fewer moles is the limiting reactant.
Step 4: Calculate the moles of C formed.
The moles of C formed will be the same as the limiting reactant since it is completely consumed in the reaction.
Step 5: Calculate the mass of C.
To calculate the mass of C, multiply the moles of C obtained in step 4 by its molar mass.
Remember, these steps are generally applicable. You need to provide the actual balanced chemical equation and molar masses of A, B, and C in order to obtain an accurate answer.
To find the mass of C, we need to apply the Law of Conservation of Mass, which states that mass cannot be created or destroyed during a chemical reaction.
Here's how you can tackle this problem:
1. Start by writing out the balanced chemical equation for the reaction between A and B, if it is given. This equation will show the stoichiometric relationship between the reactants and products.
2. Determine the molar masses of A, B, and C. To do this, find the atomic masses of each element in the compounds and multiply them by the number of atoms present. Add up these values to get the molar mass of the complete compound.
3. Convert the given masses of A and B to moles using the equation:
Moles = Mass / Molar Mass
4. Find the limiting reactant. Compare the moles of A and B to determine which reactant is in excess and which is limited. The limiting reactant is the one that produces the least number of moles of product.
5. Use the stoichiometry from the balanced equation to determine the moles of C formed. The stoichiometric coefficients in the balanced equation represent the ratio of moles between reactants and products.
6. Convert the moles of C to its mass using the equation:
Mass = Moles × Molar Mass
By following these steps, you will be able to find the mass of C formed when 1.00g of A reacts with 1.50g of B.