for instance Will write a problem. Now, I don't just want the answer, I want to know how to know which substances, and processes in steps and don't spare detail.
I am going through high school chemistry.
somehow i PAST MY Stoichiometry test. now i am ready for titration of acids and bases and need it. so instead of an over view, i need an indepth answer of how, why,and how you decide what to do and when to do it here goes if a rocket engine has 11.2 Kg of N2H4 in it, what is the minimum mas of h2o2 necessary to allow the N2H4 to react completely? so as you can see simple, except for me. i can't comprehend it. please help and don't spare detail=)
To determine the minimum mass of H2O2 needed for the N2H4 to react completely, we need to use stoichiometry and balanced chemical equations.
Let's break down the problem step by step:
1. Write the balanced chemical equation:
N2H4 + H2O2 -> N2 + 2H2O
2. Determine the molar mass of N2H4 and H2O2:
Molar mass of N2H4 = 2(N) + 4(H) = 32 g/mol
Molar mass of H2O2 = 2(H) + 2(O) = 34 g/mol
3. Convert the given mass of N2H4 to moles:
Moles of N2H4 = Mass / Molar mass
Moles of N2H4 = 11.2 kg × 1000 g/kg / 32 g/mol = 350 mol
4. Use the stoichiometry of the balanced equation to find the mole ratio between N2H4 and H2O2:
From the equation, we see that for every 1 mole of N2H4, we need 1 mole of H2O2.
Therefore, the mole ratio of N2H4 to H2O2 is 1:1.
5. Calculate the moles of H2O2 needed:
Moles of H2O2 = Moles of N2H4
Moles of H2O2 = 350 mol
6. Convert moles of H2O2 to mass:
Mass of H2O2 = Moles × Molar mass
Mass of H2O2 = 350 mol × 34 g/mol = 11,900 g
So, the minimum mass of H2O2 necessary to allow the N2H4 to react completely is 11,900 grams.
Remember, every step is crucial in solving stoichiometry problems. When faced with similar problems, follow these steps:
1. Write the balanced chemical equation.
2. Determine the molar masses of the involved compounds.
3. Convert the given mass to moles.
4. Use the stoichiometry of the balanced equation to find the mole ratio between the compounds.
5. Calculate the moles or mass of the desired substance.
6. Convert moles back to mass if necessary.
Make sure to practice more problems to strengthen your understanding of stoichiometry and continue to learn and apply these principles throughout your chemistry studies.