Question

For the reaction 2h 2 (g) + 02 (g) ~ 2h 20(1), mi~98 = -572 kj mol'. If ~ rs~98 of h20(l) is -163 j mol" k-l . Find ~ rg~98 of h20(l).

Answer 1

The Molar mass of Oxygen is 32 g/mol

Therefore moles of Oxygen = 1.6/32 =0.05

2 H2O2 = 2 H2O + O2

So, 2 x 0.05 = 0.1 moles of peroxide are needed.

The molar mass of peroxide is 34 g/mol

Mass = moles x Mr = 0.1 x 34 = 3.4g

Although in reality the yield is unlikely to be 100% so a better answer would be “more than 3.4g”

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Thanks for the A2A.

First, I would like to point out that your equation is not to the simplest form. If you want to get the correct result, you should divide everywhere by two so that we have the simplest ratio of reactants and products. The new equation is going to be:

2H2O2=====> 2H2O+O2

From the equation, we see that two moles of the the hydrogen peroxide gives us the one mole of oxygen. We can therefor say:

1 mol O2====> 16*2=32g

0.05 mol ====>1.6g

1 mol O2 ===>2 mol H2O2

0.05 mol ===>0.1 mol

1 mol H2O2 ===> 2+32=34g

0.1 mol======> 0.1*34 =3.4g

So, 3.4g are needed to produce the 1.6g of Oxygen

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hii friends i am aditya

The Molar mass of Oxygen is 32 g/mol

Therefore moles of Oxygen = 1.6/32 =0.05

2 H2O2 = 2 H2O + O2

So, 2 x 0.05 = 0.1 moles of peroxide are needed.

The molar mass of peroxide is 34 g/mol

Mass = moles x Mr = 0.1 x 34 = 3.4g

Although in reality the yield is unlikely to be 100% so a better answer would be “more than 3.4g