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 .

38 L

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.

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.

the volume increases

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.