Question

How many liters of hydrogen gas are needed to produce 130.0 grams of water at 25.0¬[infinity]C and 1.00 atm pressure according to the chemical equation shown below?

Answer 1

To find the mass of H2O2 solution needed to produce O2 gas, calculate the moles of oxygen using the balanced chemical equation and the molar mass of H2O2. Then, convert the moles of H2O2 to grams using its molar mass.

Step-by-step explanation:

To find the mass of H2O2 solution needed to produce 35.7 g of O2(g), we need to first calculate the moles of oxygen using the balanced chemical equation. From the equation, we can see that 1 mole of H2O2 produces 1 mole of O2 gas. Therefore, the moles of O2 gas is equal to the moles of H2O2. Next, we can calculate the moles of H2O2 using its molar mass.

Once we have the moles of H2O2, we can convert it to grams using its molar mass. The mass of 3.00% H2O2 solution can then be calculated using the mass-to-mole ratio.

Answer 2

The volume (in liters) of hydrogen gas needed to produce 130.0 grams of water is 176.64 liters

How to calculate the volume of hydrogen needed?

We shall begin by calculating the number of mole of water produced from the reaction. This is shown below:

• Mass of water produced = 130.0 grams
• Molar mass of water = 18 g/mol
• Mole of water produced =?

Mole of water produced = mass / molar mass

= 130 / 1 8

= 7.22 moles

Now, we shall calculate the mole of hydrogen needed to produced 7.22 moles (i.e 130 grams) of water.

`2H_2(g)\ +\ O_2(g)\ \rightarrow\ 2H_2O(g)`

From the balanced equation above,

2 moles of water were produced from 2 moles of hydrogen

Therefore,

7.22 moles of water will also be produced from 7.22 moles of hydrogen

With the mole of hydrogen gas obtained above, we shall calculate the volume of hydrogen gas needed for the reaction. Details below:

• Temperature (T) = 25 °C = 25 + 273 = 298 K
• Pressure (P) = 1.00 atm
• Gas constant (R) = 0.0821 atm.L/mol K
• Number of mole (n) = 7.22 moles
• Volume of hydrogen gas (V) =?

PV = nRT

1 × V = 7.22 × 0.0821 × 298

V = 176.64 liters

Complete question:

How many liters of hydrogen gas are needed to produce 130.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below?

2H₂(g) + O₂(g) → 2H₂O(g)