Hydrogen peroxide, h2o2, in the presence of a catalyst decomposes into water and oxygen gas. how many l of o2 at stp are produced from the decomposition of 34.0g of h2o2? a.) 1.00b.) 5.60c.) 11.2d.) 22.4

There is 11.2 L of O2 produced

Explanation:

Step 1: Data given

Molar mass of H2O2 = 34.01 g/mol

Molar mass of O2 = 32 g/mol

Mass of H2O2 = 34.0 grams

Step 2: The balanced reaction

2H2O2 → 2H2O + O2

Step 3: Calculate number of moles H2O2

Moles H2O2 = Mass H2O2 / Molar mass H2O2

Moles H2O2 = 34 grams / 34.01 g/mol

Moles H2O2 = 1 mol

Step 4: Calculate the number of moles at the equilibrium

Initial number of moles H2O2 = 1 mol

Initial number of mol H2O and O2 = 0 mol

Since the mol ratio H2O2 H2O O2 is 2:2:1

There will react x mol of H2O2; X mol of H2O and 0.5 x mol of O2

At the equilibrium, H2O2 has (1-x) mol. Since it's decomposed into H2O and O2, we know x =1 mol

At the equilibrium, there is 1 mol H2O and 0.5 mol O2

Under STP, 1 mol of gas has a volume of 22.4 L

This means 0.5 moles of O2 has a volume of 22.4*0.5 = 11.2 L

There is 11.2 L of O2 produced

c)red bank

explanation:

red bank is a borough in monmouth county, new jersey, incorporated in 1908 and located on the navesink river, the area's original transportation route to the ocean and other ports.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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