Upon decomposition, one sample of magnesium fluoride produced 1.64 kg of magnesium and 2.57 kg of fluorine. A second sample produced 1.38 kg of magnesium.

How much fluorine (in grams) did the second sample produce?

I don't know what procedure you are to use. The following is not a mole ratio type solution.

2.57 kg x (1.38/1.64) = ?? kg F2.

2.162560976

To determine the amount of fluorine produced by the second sample, we need to find the ratio of magnesium to fluorine in the first sample and then apply it to the amount of magnesium in the second sample.

Given:
First sample - 1.64 kg of magnesium and 2.57 kg of fluorine.
Second sample - 1.38 kg of magnesium.

Step 1: Find the ratio of magnesium to fluorine in the first sample.
Since the first sample produced 1.64 kg of magnesium and 2.57 kg of fluorine, we can calculate the ratio of magnesium to fluorine as:
ratio = mass of magnesium / mass of fluorine = 1.64 kg / 2.57 kg.

Step 2: Apply the ratio to the amount of magnesium in the second sample.
Since the second sample produced 1.38 kg of magnesium, we can calculate the amount of fluorine produced by multiplying the mass of magnesium in the second sample with the ratio obtained from step 1:
fluorine produced = mass of magnesium (second sample) * ratio.

Let's perform the calculations:
ratio = 1.64 kg / 2.57 kg ≈ 0.638 ratio (rounded to three decimal places)
fluorine produced = 1.38 kg * 0.638 ≈ 0.881 kg (rounded to three decimal places)

To convert the kilograms to grams, we can multiply by 1000:
0.881 kg * 1000 = 881 grams.

Therefore, the second sample produced approximately 881 grams of fluorine.