Question

How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K .

Answer 1

38 L

Step-by-step explanation:

There is some info missing. I think this is the original question.

Consider the chemical reaction: C(s) + H₂ O(g) ⟶ CO(g) + H₂ (g). How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K.

Step 1: Write the balanced equation

C(s) + H₂ O(g) ⟶ CO(g) + H₂ (g)

Step 2: Calculate the moles corresponding to 15.2 g of C

The molar mass of C is 12.01 g/mol.

`15.2g * (1mol)/(12.01g) = 1.27 mol`

Step 3: Calculate the moles of H₂ produced from 1.27 moles of C

The molar ratio of H₂ to C is 1:1. The moles of H₂ produced are 1/1 × 1.27 mol = 1.27 mol.

Step 4: Calculate the volume of H₂

We will use the ideal gas equation.

`P * V = n * R * T\\V = (n * R * T)/(P) = (1.27mol * (0.0821atm.L)/(mol.K) * 360K)/(1.0atm)= 38 L`