The orbits of the planets in our solar system arenot
a Elliptical, circular
b Circular, elliptical
C Circular, oval
d None of the above

Answer:

3.16 × 10−8

Explanation:

Answer:

The partial pressure of  nitrogen is  0.402 atm.

Explanation:

Given data:

Number of moles of helium = 1 mol

Number of moles of nitrogen = 2 mol

Total pressure of mixture = 0.60 atm

Partial pressure of nitrogen = ?

Solution:

First of all we will calculate the mole fraction of nitrogen.

mole fraction of nitrogen = moles of nitrogen / total number of moles

mole fraction of nitrogen = 2 mol / 3 mol = 0.67

Partial pressure of nitrogen:

P₁ = [ n₁ /n(t)] × Pt

P₁ = 0.67 × 0.60 atm

P₁ = 0.402 atm

Final answer:

To find the partial pressure of nitrogen in a mixture, calculate the mole fraction of nitrogen and multiply it by the total pressure of the mixture. In this case, the partial pressure of nitrogen is 0.40 atm.

Explanation:

The question is about determining the partial pressure of nitrogen in a mixture of helium and nitrogen based on Dalton's Law of Partial Pressures. First, we find the mole fraction of nitrogen, which is the ratio of moles of nitrogen to the total moles in the mixture. In this scenario, the mole fraction (XN2) is 2 moles of nitrogen divided by the total moles (1 mole of helium + 2 moles of nitrogen), which equals 2/3.

Then we use Dalton's Law, which states that the partial pressure of nitrogen (PN2) can be found by multiplying the mole fraction by the total pressure of the mixture. Therefore, the partial pressure of nitrogen is 0.60 atm (total pressure) multiplied by 2/3 (mole fraction of nitrogen), yielding a partial pressure for nitrogen of 0.40 atm.

Learn more about partial pressure here:

brainly.com/question/31214700

#SPJ3

Answer:

Mn: 3+

Cl: 7+

O: 2-

Explanation:

1) Compound given: Mn [ClO₄]₃

2) Initially you only know the oxidation state of O, since it is always 2-, except when it form peroxides, which is not the case.

3) So, you do not know the oxidation states neither of the Mn nor of the Cl, and you need some more information.

You might start from the ion [ClO₄] but you do not know its charge.

This ion comes from one of the oxoacids formed by Cl. Those are four different acids. These are them:

i) Oxidation state 1+: Cl₂O + H₂O → H₂Cl₂O₂ = HClO ⇒ ion ClO⁻

ii) Oxidation state 3+: Cl₂O₃ + H₂O → H₂Cl₂O₄ = HClO₂ ⇒ ion ClO₂⁻

iii) Oxidation state 5+: Cl₂O5 + H₂O → H₂Cl₂O₆ = HClO₃ ⇒ ion ClO₃⁻

iv) Oxidation state 7+: Cl₂O₇ + H₂O → H₂Cl₂O₈ = HClO₄ ⇒ ion ClO₄⁻

Finally, we have that our ion is ClO₄⁻ and the oxidation state of Cl is 7+.

4) Now you just have to find the oxidation state of Mn, for which you make a balance of charges:

Mn [ClO₄]₃

Since, the ion ClO₄⁻ has 1 negative charge, and there are 3 ions the total negative charge is 3-. Since the compound is neutral, you conclude that Mn has oxidation state 3+.

That according to this balance: 1(3+) + 3(1-) + 3 - 3 = 0.

5) Summarizing, the oxidation states are:

Mn: 3+

Cl: 7+

O: 2-