Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition.

2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ
How much heat is released when 529 kg H2O2 decomposes?

( ......... ) KJ

*note ..watch sig figs .

my work:
• 2 H2O2(l) => 2 H2O(l) + O2(g) ΔHrxn = -196.1 kJ
Moles of H2O2 = mass/molar mass
= 529,000/34 = 15558.82 moles of H2O2 release 196.1 kJ of heat
Total heat released = 15558.82/2 x196.1 = 1525542.301 = 1.52554 × 10^6
= 1.53 x 10^6 kJ (3 significant figures)
am I correct?.....thank you.

Yes, your calculations are correct. To calculate the heat released when 529 kg of H2O2 decomposes, we can follow these steps:

1. Determine the moles of H2O2: The molar mass of H2O2 is 34 g/mol. To convert 529 kg to grams, we multiply by 1000: 529 kg * 1000 g/kg = 529,000 g. Then divide the mass by the molar mass: 529,000 g / 34 g/mol = 15,558.82 mol.

2. Use the stoichiometry of the reaction: From the balanced equation, we can see that 2 moles of H2O2 produce 196.1 kJ of heat. Therefore, 1 mole of H2O2 will produce 196.1 kJ / 2 = 98.05 kJ of heat.

3. Calculate the total heat released: Multiply the moles of H2O2 by the heat produced per mole: 15,558.82 mol * 98.05 kJ/mol = 1,525,542.3 kJ.

4. Apply significant figures: The given value, 529 kg, has 3 significant figures. Therefore, the final answer should also have 3 significant figures. Rounding to three decimal places, the heat released is 1.53 × 10^6 kJ.

So, the correct answer is approximately 1.53 × 10^6 kJ.

Yes, you are correct. Your calculations are accurate.

To find the moles of H2O2, you divide the mass of H2O2 by its molar mass:

529 kg H2O2 x (1000 g/ 1 kg) / (34.02 g/mol) = 15558.82 moles of H2O2

Since the stoichiometric ratio between H2O2 and heat released is 2:1, you only need to consider half of the moles of H2O2 when calculating the heat released:

Heat released = (15558.82 moles of H2O2 / 2) * (-196.1 kJ/mol)
= 1.5255426 x 10^6 kJ

Rounded to 3 significant figures, the heat released is 1.53 x 10^6 kJ. Good job!