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
see below
Sorry for this question is incomplete coz molecular weight not given
To determine how many grams of C and D should be obtained, we need to use stoichiometry. Stoichiometry is the calculation of the quantities of reactants and products involved in a chemical reaction.
In the given balanced chemical equation:
1A + 3B -> 2C + 4D
We can see that 1 mole of A reacts with 3 moles of B to produce 2 moles of C and 4 moles of D. The molar masses of substances A, B, C, and D will be required to solve this problem.
Let's assume the molar masses of A, B, C, and D are MA, MB, MC, and MD, respectively.
To get the number of moles of A and B used in the reaction, we need to convert the given masses to moles using the formula:
Number of moles = mass / molar mass
moles of A = 5.0g / MA
moles of B = 6.0g / MB
Using the balanced chemical equation, we can establish a mole ratio between A, B, C, and D:
1 mole A : 3 moles B : 2 moles C : 4 moles D
Now, to find the number of moles of C and D produced, we can use these ratios:
moles of C = (moles of A) x (2 moles C / 1 mole A)
moles of D = (moles of A) x (4 moles D / 1 mole A)
After calculating the moles of C and D, we can convert them back to grams by multiplying with their respective molar masses:
grams of C = (moles of C) x MC
grams of D = (moles of D) x MD
Finally, we will have the values of grams of C and D obtained in the reaction.
Without the molar masses of A, B, C, and D or any other relevant information, it is not possible to determine the exact values of grams of C and D. Therefore, the answer is: "Not enough information to answer the question."