# It is required to make grams of certain chemical compound called . this is made from compounds , , and in the ratio of . the compound is itself made from and . to make grams of requires grams of and grams of . how much and is required to make the required amount of?

Question: It is required to make grams of certain chemical compound called . this is made from compounds , , and in the ratio of . the compound is itself made from and . to make grams of requires grams of and grams of . how much and is required to make the required amount of?

We will learn how to calculate the amount of reactants needed to produce a certain amount of a chemical compound. The compound we are interested in is called X, and it is made from compounds A, B, and C in the ratio of 2:3:4. The compound A is itself made from D and E. To make 10 grams of A, we need 6 grams of D and 4 grams of E. How much D and E is required to make 100 grams of X?

To answer this question, we need to use the concept of stoichiometry, which is the study of the quantitative relationships between reactants and products in a chemical reaction. Stoichiometry allows us to determine the amount of a substance that is consumed or produced in a reaction based on the balanced chemical equation and the mole ratios.

The first step is to write the balanced chemical equation for the synthesis of X from A, B, and C. We can assume that the reaction goes to completion, meaning that all the reactants are converted into products. The equation is:

2A + 3B + 4C -> X

The second step is to convert the given mass of X (100 grams) into moles using its molar mass. The molar mass is the mass of one mole of a substance, and it can be calculated by adding up the atomic masses of all the elements in the compound. For example, if X has the formula C6H12O6, its molar mass is:

(6 x 12) + (12 x 1) + (6 x 16) = 180 g/mol

We can use this value to find the number of moles of X by dividing the mass by the molar mass:

n(X) = m(X) / M(X) = 100 / 180 = 0.556 mol

The third step is to use the mole ratio from the balanced equation to find the number of moles of A that are needed to produce 0.556 moles of X. The mole ratio is the ratio of coefficients in front of each substance in the equation. For example, the mole ratio of A to X is 2:1, meaning that for every mole of X produced, two moles of A are consumed. We can use this ratio to set up a proportion and solve for n(A):

n(A) / n(X) = 2 / 1

n(A) = n(X) x (2 / 1)

n(A) = 0.556 x 2

n(A) = 1.111 mol

The fourth step is to convert the number of moles of A into mass using its molar mass. We can use the same method as before, but in reverse. For example, if A has the formula CH4, its molar mass is:

(1 x 12) + (4 x 1) = 16 g/mol

We can use this value to find the mass of A by multiplying the number of moles by the molar mass:

m(A) = n(A) x M(A) = 1.111 x 16 = 17.78 g

The fifth and final step is to repeat steps three and four for D and E, using their respective mole ratios and molar masses. For example, if D has the formula O2 and E has the formula H2, their molar masses are:

(2 x 16) = 32 g/mol

(2 x 1) = 2 g/mol

And their mole ratios with A are:

D : A = 3 : 2

E : A = 4 : 2

We can use these values to find the masses of D and E by following the same procedure as before:

m(D) = n(D) x M(D)

n(D) = n(A) x (3 / 2)

m(D) = n(A) x (3 / 2) x M(D)

m(D) = 1.111 x (3 / 2) x 32

m(D) = 53.33 g

m(E) = n(E) x M(E)

n(E) = n(A) x (4 / 2)

m(E) = n(A) x (4 / 2) x M(E)

m(E) = 1.111 x (4 / 2) x 2

m(E) = 4.44 g

Therefore, to make 100 grams of X, we need:

53.33 grams of D

4.44 grams of E

17.78 grams of A

and some unknown amounts of B and C.

We hope this blog post was helpful and informative. If you have any questions or comments, please feel free to leave them below.

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