elemental sulfur can bea formed through the combustion of hydrogen sulfide (found in methane gas) carve in equation; H2 S +O2----S + H2 4

tell how much sulfur is made from 250 grams of methane

You need to redo your typing job, especially for "carve", H2 S and H2 4. None of that makes sense to me. Also, I don't see methane anywhere in the equation and nothing that tells me the percent S in methane.

A 0.250 g sample of a gas occupies 0.100 L at a pressure of 2.50 atm and a temperature of 25.0ºC. What molar mass?

To determine how much sulfur is produced from the combustion of 250 grams of methane, we need to use the given balanced chemical equation as a reference.

The balanced equation is:

H2S + O2 → S + H2O

From the equation, we can see that the stoichiometric ratio between hydrogen sulfide (H2S) and sulfur (S) is 1:1. This means that for every 1 mole of H2S, 1 mole of S is produced.

To calculate the amount of sulfur produced, we need to follow these steps:

Step 1: Convert the mass of methane (CH4) to moles.
To do this, we need the molar mass of methane, which is 16.04 g/mol (1C:12.01 g/mol + 4H:1.01 g/mol).

Moles of CH4 = mass of CH4 / molar mass of CH4
Moles of CH4 = 250 g / 16.04 g/mol ≈ 15.58 moles

Step 2: Use the stoichiometric ratio to determine the number of moles of sulfur produced.
From the balanced equation, we know that the ratio of moles of H2S to moles of S is 1:1.
Therefore, 15.58 moles of H2S will produce 15.58 moles of S.

Step 3: Convert moles of sulfur to grams.
To do this, we need the molar mass of sulfur, which is 32.06 g/mol.

Mass of S = moles of S × molar mass of S
Mass of S = 15.58 mol × 32.06 g/mol ≈ 499.63 g

Therefore, approximately 499.63 grams of sulfur are produced from the combustion of 250 grams of methane.