A reastion consumes 5.0g of A and 6.0g of B. How many grams of C and D should be obtained?
1A + 3B -> 2C + 4D
MC answers:
23
11
1
10
Not enough information to answer the question
With moles A and B reacting you might get somewhere but with grams and no way to convert to moles?
To determine the amount of grams of C and D obtained in the reaction, we need to use the stoichiometry of the balanced chemical equation.
According to the balanced equation: 1A + 3B → 2C + 4D
First, we need to calculate the limiting reactant by comparing the moles of A and B. To do this, we convert the given masses of A and B to moles using their molar masses.
Molar mass of A = M
Molar mass of B = N
Moles of A = 5.0g / M
Moles of B = 6.0g / N
Next, we compare the ratios of A and B in the balanced equation to determine which reactant is the limiting reactant. Since the coefficients of A and B are 1 and 3, respectively, we can calculate the ratio of moles of A to moles of B required for the reaction.
Moles of A / Coefficient of A = (5.0g / M) / 1 = 5.0g / M
Moles of B / Coefficient of B = (6.0g / N) / 3 = 2.0g / (3N)
Comparing the two ratios, if 5.0g/M < 2.0g/(3N), then A is the limiting reactant. If the opposite is true, B is the limiting reactant.
Now, we can determine the moles of C and D produced from the limiting reactant. According to the stoichiometry of the balanced equation, the molar ratio of A to C is 1:2 and B to D is 3:4.
Moles of C = Moles of A * (2 moles of C / 1 mole of A)
Moles of D = Moles of B * (4 moles of D / 3 moles of B)
Finally, we can calculate the mass of C and D by multiplying the moles obtained by their respective molar masses.
Mass of C = Moles of C * Molar mass of C
Mass of D = Moles of D * Molar mass of D
Please provide the molar masses of C and D or the values of M and N so that I can provide you with the specific answer.