Get comprehensive solutions to your problems with IDNLearn.com. Get thorough and trustworthy answers to your queries from our extensive network of knowledgeable professionals.
Sagot :
Sure, let's solve the problem by analyzing the balanced chemical equation:
[tex]\[ N_2H_4 + 2 H_2O_2 \rightarrow N_2 + 4 H_2O \][/tex]
We need to determine the mole ratios of hydrazine ([tex]\(N_2H_4\)[/tex]) to hydrogen peroxide ([tex]\(H_2O_2\)[/tex]), and hydrazine to water ([tex]\(H_2O\)[/tex]) from this equation.
1. Mole Ratio of N_2H_4 to H_2O_2:
- According to the balanced equation, 1 mole of [tex]\(N_2H_4\)[/tex] reacts with 2 moles of [tex]\(H_2O_2\)[/tex].
- Therefore, the mole ratio of [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O_2\)[/tex] is:
[tex]\[ \frac{1 \text{ mole } N_2H_4}{2 \text{ moles } H_2O_2} = 1:2 \][/tex]
2. Mole Ratio of N_2H_4 to H_2O:
- According to the balanced equation, 1 mole of [tex]\(N_2H_4\)[/tex] produces 4 moles of [tex]\(H_2O\)[/tex].
- Therefore, the mole ratio of [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O\)[/tex] is:
[tex]\[ \frac{1 \text{ mole } N_2H_4}{4 \text{ moles } H_2O} = 1:4 \][/tex]
So, the correct mole ratios are:
- [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O_2\)[/tex]: [tex]\(1:2\)[/tex]
- [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O\)[/tex]: [tex]\(1:4\)[/tex]
Matching these ratios with the given choices:
- [tex]\(1:2\)[/tex] and [tex]\(1:4\)[/tex]
- [tex]\(4i3\)[/tex] and [tex]\(1.8\)[/tex]
- [tex]\(1:2\)[/tex] and [tex]\(3:5\)[/tex]
The correct choice is:
[tex]\[ \boxed{1:2 \text{ and } 1:4} \][/tex]
[tex]\[ N_2H_4 + 2 H_2O_2 \rightarrow N_2 + 4 H_2O \][/tex]
We need to determine the mole ratios of hydrazine ([tex]\(N_2H_4\)[/tex]) to hydrogen peroxide ([tex]\(H_2O_2\)[/tex]), and hydrazine to water ([tex]\(H_2O\)[/tex]) from this equation.
1. Mole Ratio of N_2H_4 to H_2O_2:
- According to the balanced equation, 1 mole of [tex]\(N_2H_4\)[/tex] reacts with 2 moles of [tex]\(H_2O_2\)[/tex].
- Therefore, the mole ratio of [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O_2\)[/tex] is:
[tex]\[ \frac{1 \text{ mole } N_2H_4}{2 \text{ moles } H_2O_2} = 1:2 \][/tex]
2. Mole Ratio of N_2H_4 to H_2O:
- According to the balanced equation, 1 mole of [tex]\(N_2H_4\)[/tex] produces 4 moles of [tex]\(H_2O\)[/tex].
- Therefore, the mole ratio of [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O\)[/tex] is:
[tex]\[ \frac{1 \text{ mole } N_2H_4}{4 \text{ moles } H_2O} = 1:4 \][/tex]
So, the correct mole ratios are:
- [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O_2\)[/tex]: [tex]\(1:2\)[/tex]
- [tex]\(N_2H_4\)[/tex] to [tex]\(H_2O\)[/tex]: [tex]\(1:4\)[/tex]
Matching these ratios with the given choices:
- [tex]\(1:2\)[/tex] and [tex]\(1:4\)[/tex]
- [tex]\(4i3\)[/tex] and [tex]\(1.8\)[/tex]
- [tex]\(1:2\)[/tex] and [tex]\(3:5\)[/tex]
The correct choice is:
[tex]\[ \boxed{1:2 \text{ and } 1:4} \][/tex]
We appreciate your contributions to this forum. Don't forget to check back for the latest answers. Keep asking, answering, and sharing useful information. IDNLearn.com is your reliable source for accurate answers. Thank you for visiting, and we hope to assist you again.