If 175mL of oxygen is produced at STP, how many grams of hydrogen peroxide, H2O2

were decomposed? At STP, 1 mole of gas occupies 22.4L. Be sure to balance first.

2 H202 > H202 + O2

what's the

Mass of H2O2

0.53g

Explanation:

We'll begin by converting 175mL to L. This is illustrated below:

1000mL = 1L

Therefore 175mL = 175/1000 = 0.175L

Next, we shall calculate the number of mole of O2 that occupy 0.175L. This is illustrated below:

1 mole of O2 occupy 22.4L at stp.

Therefore, Xmol of O2 will occupy 0.175L i. e

Xmol of O2 = 0.175/22.4

Xmol of O2 = 7.81*10¯³ mole

Therefore, 7.81*10¯³ mole of O2 occupy 175mL.

Next, we shall determine the number of mole of H2O2 that decomposed to produce 7.81*10¯³ mole of O2. This is illustrated below:

2H2O2 - > 2H2O + O2

From the balanced equation above,

2 moles of H2O2 decomposed to produce 1 mole of O2.

Therefore, Xmol of H2O2 will decompose to produce 7.81*10¯³ mole of O2 i. e

Xmol of H2O2 = 2 x 7.81*10¯³

Xmol of H2O2 = 1.562*10¯² mole

Therefore, 1.562*10¯² mole of H2O2 decomposed in the reaction.

Finally, we shall convert 1.562*10¯² mole of H2O2 to grams. This is illustrated below:

Molar mass of H2O2 = (2x1) + (16x2) = 34g/mol

Mole of H2O2 = 1.562*10¯² mole

Mass of H2O2 = ... ?

Mole = mass / Molar mass

1.562*10¯² = mass / 34

Cross multiply

Mass of H2O2 = 1.562*10¯² x 34

Mass of H2O2 = 0.53g

Therefore, 0.53g of Hydrogen peroxide, H2O2 were decomposition in the reaction.