What weight of H2 at STP could be contained in a vessel that holds 4g of oxygen at STP?

First, I used the Ideal Gas Law to find the volume of oxygen at STP, but im not sure what to do from there..

To find the weight of hydrogen, you can follow these steps:

1. Begin by determining the number of moles of oxygen. This can be done using the ideal gas law, PV = nRT, where P is the pressure (which is 1 atm at standard temperature and pressure or STP), V is the volume of oxygen, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature (which is 273.15 K at STP).

2. Rearrange the ideal gas law to solve for the number of moles (n). The equation becomes n = PV / RT. Insert the values P = 1 atm, V = volume of oxygen (which is previously calculated), R = 0.0821 L·atm/(mol·K), and T = 273.15 K, and solve for n.

3. Now, determine the molar ratio between oxygen (O2) and hydrogen (H2) using the balanced chemical equation for the reaction between the two: 2H2 + O2 → 2H2O. The ratio shows that for every 1 mole of oxygen, 2 moles of hydrogen are required to react.

4. Multiply the number of moles of oxygen by the molar ratio of hydrogen to oxygen to determine the number of moles of hydrogen gas.

5. Finally, calculate the weight of hydrogen by multiplying the number of moles of hydrogen gas by the molar mass of hydrogen, which is approximately 2 g/mol.

By following these steps, you will be able to calculate the weight of hydrogen that could be contained in the vessel.

Use PV = nRT again. You know volume from the previous work, then plug in R, T, and P, calculate n for H2. Then moles = grams/molar mass will allow you to calculate grams.