Question

A group of students used 5.6 grams of sulfide to complete the above reaction. They claim that you can get 7.56 grams of magnesium sulfide from that amount. Is this possible?

A) Yes, the claim is correct.
B) No, the claim is not correct.

Answer 1

The claim is not correct because the theoretical yield of magnesium sulfide is greater than the claimed yield.

Step-by-step explanation:

In order to determine if the claim is correct, we need to calculate the theoretical yield of magnesium sulfide based on the reaction. From the given information, we know that 5.6 grams of sulfide was used. Using the molar mass of sulfur (32.07 g/mol), we can convert grams of sulfide to moles of sulfide:

5.6 g Sulfide x (1 mol Sulfur / 32.07 g Sulfur) = 0.175 mol Sulfur

Using the balanced equation for the reaction, which states that 1 mole of sulfur reacts with 1 mole of magnesium to produce 1 mole of magnesium sulfide, we can determine the theoretical yield of magnesium sulfide:

0.175 mol Sulfur x (1 mol Magnesium Sulfide / 1 mol Sulfur) x (56.30 g Magnesium Sulfide / 1 mol Magnesium Sulfide) = 9.86 g Magnesium Sulfide

Since the theoretical yield of magnesium sulfide is greater than the claimed yield of 7.56 grams, the claim is not correct. Therefore, the correct answer is option B) No, the claim is not correct.