Question

A chemist is preparing to carry out a reaction at high pressure that requires 36.0 moles of hydrogen gas. The chemist pumps the hydrogen into a 12.4 L rigid steel container at 25.0oC. To what pressure, in atm, must the hydrogen be compressed? a. What gas law applies to this scenario? b. Solve for the unknown variable (include the units in your answer).

Answer 1

To find the pressure, we can use the ideal gas law and rearrange the equation to solve for pressure. Plugging in the given values, we find that the pressure must be compressed to 68.99 atm.

Step-by-step explanation:

To solve this problem, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.0821 L atm/mol K), and T is the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin by adding 273.15. So, 25.0°C is equal to 298.15 K.

Using the given information, we can rearrange the ideal gas law equation to solve for pressure. P = (nRT) / V

Plugging in the values, we have P = (36.0 mol * 0.0821 L atm/mol K * 298.15 K) / 12.4 L

Solving this equation gives us P = 68.99 atm.