Question

A container contains 32 g of O₂ at a temperature TThe pressure of the gas is P. An identical containercontaining 4 g of H₂ at a temperature 2T has apressure of

(1) 8P
(2) 4P
(3) P
(4) P18r-cnstant

Answer 1

To find the pressure of the hydrogen gas, we can use the ideal gas law equation and convert the given masses of oxygen and hydrogen to moles. The pressure of the hydrogen gas is 4P. Therefore, the correct option is 2.

Step-by-step explanation:

To solve this problem, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. In this case, we are given the amount of oxygen and hydrogen in grams, but we need to convert it to moles. We can use the molar mass of each element to calculate the number of moles. We can then substitute the values into the ideal gas law equation to find the pressure of the hydrogen gas.

We know that the volume and temperature are the same for both containers, so the only difference is the number of moles of gas. Therefore, the pressure of the hydrogen gas is 4P.

Hence, the answer is option (2) 4P.