A gas contains a mixture of NH3(g) and N2H4(g), both of which react with O2(g) to form NO2(g) and H2O(g). The gaseous mixture (with an initial mass of 61.00 g) is reacted with 10.00 moles O2, and after the reaction is complete, 4.062 moles O2 remains. Calculate themass percent of N2H4(g) in the original gaseous mixture.
Answers
Answer:
Mass percent of N2H4 in original gaseous mixture = 31.13 %
Explanation:
Given:
Initial mass of gaseous mixture = 61.00 g
Initial mole of oxygen = 10.0 mol
Moles of oxygen remaining after the reaction = 4.062 mol
Moles of oxygen used = 10.0 - 4.062 = 5.938 mol
Total oxygen used in both the reactions = 10.0 parts
out of 10 parts, 3 part react with N2H4.
Now, consider the reaction of N2H4
3 moles of O2 react with 1 mole of N2H4
1.78 moles of oxygen will react with 1.78/3 = 0.5933 mol of N2H4
Molecular mass of N2H4 = 32 g/mol
Total mass = 61.0 g
Final answer:
The mass percent of N2H4 in the gaseous mixture can be determined through stoichiometric calculations and determining the limiting reactant. The initial and remaining amounts of O2 are used to calculate the reacted amount of O2, which then allows for the calculation of the amount of N2H4. This information is used in the mass percent formula.
Explanation:
The balanced reaction states that for one mole of NH3, one mole of O2 is required, while for one mole of N2H4, 3 moles of O2 are required. Thus, the initial moles of O2 were 10 moles and after reaction 4.062 moles O2 remained. Thus, the reacted amount of O2 is 10 - 4.062 = 5.938 moles. From calculating the limiting reactant and applying stoichiometry, the amount of N2H4 can be determined. We know the molar mass of N2H4 is 32 g/mole. By calculating the molar ratio, we can then calculate the mass percent of N2H4 in the mixture using the formula: (mass of N2H4 / total mass) * 100%.
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Answer:
Answers
A star is born, it radiates energy for a long time, toward the end it expands, it may or may not explode, and then it dies. It vary in sizes, masses and surface temperature range. The colors of stars reflect their surface temperature. Their relative brightness is expressed in a scale of six magnitudes. The brightest the stars are first-magnitude stars, while the dimmest are sixth-magnitude stars.
The lower the number, the brighter the star.
For example:
Star color Surface Temperature
Blue-white around 25 000 K & higher
white around 10 000 K
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2.) Al^3+, O^2-
3.) Ca^2, ClO3-
4.) NH4+, P^3-
5.) Cu+, NO3-
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Answer:
1.) NiSO₄; 2.) Al₂O₃; 3.) Ca(ClO₃)₂; 4.) (NH₄)₃P; 5.) CuNO₃
Step-by-step explanation:
We can use the criss-cross method to work out the formulas. The steps are
- Write the symbols of the anion and cation.
- Criss-cross the numbers of the charges to become the subscripts of the other ion (as in the image).
- Write the formula with the new subscripts.
- Divide the subscripts by their highest common factor.
- Omit all subscripts that are 1.
If we use this method, the formula for the compound formed from Na⁺, SO₃²⁻ becomes Na₂SO₃.
1.) Ni²⁺ + SO₄²⁻ ⟶ Ni₂(SO₄)₂ ⟶ NiSO₄
2.) Al³⁺ + O²⁻ ⟶ Al₂O₃
3.) Ca²⁺ + ClO₃⁻ ⟶ Ca(ClO₃)₂
4.) NH₄⁺ + P³⁻ ⟶ (NH₄)₃P
5.) Cu⁺ + NO₃⁻ ⟶ CuNO₃
2) empirical formulas
3) molecular structures
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Answers
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