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2 years ago

15

Which of the following is a valid conversion factor?

2 answers:

VMariaS [17]2 years ago

7 0

Answer:

100 cg/1g

Step-by-step explanation:

1 cg = 0.01 g Multiply by 100

100 cg = 1 g

(a) is <em>wrong</em>. The correct conversion factor is 1000 cm³/1 L.

(b) is <em>wrong</em>. The correct conversion factor is 1000 mL/1 L.

(c) is <em>wrong</em>. The correct conversion factor is 1 m/10 dm.

telo118 [61]2 years ago

4 0

Answer:

100 centigrams over one gram

Explanation:

<em>Which of the following is a valid conversion factor?</em>

<em>one cubic centimeter over one liter</em> FALSE

According to the International System of Units, 1 cm³ = 1mL.

<em>one milliliter over 100 liters</em> FALSE

The prefix mili- corresponds to 10⁻³.

Thus, 1 mL = 10⁻³ L = 0.001 L

<em>10 meters over one decimeter</em> FALSE

The prefix deci- corresponds to 10⁻¹.

Thus, 1 dm = 10⁻¹ m = 0.1 m

<em>100 centigrams over one gram</em> TRUE

The prefix centi- corresponds to 10⁻².

Thus,

1 cg = 10⁻² g = 0.01 g

100 cg = 1 g

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If an aqueous solution of urea n2h4co is 26% by mass and has density of 1.07 g/ml, calculate the molality of urea in the soln

Ksju [112]

Answer is: molality of urea is 5.84 m.

If we use 100 mL of solution:
d(solution) = 1.07 g/mL.
m(solution) = 1.07 g/mL · 100 mL.
m(solution) = 107 g.
ω(N₂H₄CO) = 26% ÷ 100% = 0.26.
m(N₂H₄CO) = m(solution) · ω(N₂H₄CO).
m(N₂H₄CO) = 107 g · 0.26.
m(N₂H₄CO) = 27.82 g.
1) calculate amount of urea:
n(N₂H₄CO) = m(N₂H₄CO) ÷ M(N₂H₄CO).
n(N₂H₄CO) = 27.82 g ÷ 60.06 g/mol.
n(N₂H₄CO) = 0.463 mol; amount of substance.
2) calculate mass of water:
m(H₂O) = 107 g - 27.82 g.
m(H₂O) = 79.18 g ÷ 1000 g/kg.
m(H₂O) = 0.07918 kg.
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2 years ago

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The combustion of propane occurs when propane interacts with oxygen gas to produce water and carbon dioxide in the following rea

gtnhenbr [62]

Answer:

20 atm

Explanation:

<u>1) Data:</u>

a) n = 2 moles

b) T = 373 K

c) V = 2.5 liter

d) P = ?

<u>2) Chemical principles and formula</u>

You need to calculate the pressure of the propane gas in the mixture before reacting. So, you can apply the partial pressure principle which states that each gas exerts a pressure as if it occupies the entire volume.

Thus, you just have to use the ideal gas equation: PV = nRT

<u>3) Solution:</u>

PV = nRT ⇒ P = nRT / V

P = 2 mol × 0.08206 atm-liter /K-mol × 373K / 2.5 liter = 24.5 atm

Since the number of moles are reported with one significant figure, you must round your answer to one significant figure, and that is 20 atm (20 is closer to 24.5 than to 30).

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5. Gabi has plans with her friends to go to a concert on her birthday in 4 days. She is so excited that she wants to know how ma

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Answer:

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Explanation:

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60 minute = 1 hour

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3600 second * 24 hours =

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When adjusted for any changes in ΔHΔH and ΔSΔS with temperature, the standard free energy change ΔG∘TΔGT∘Delta G_{T}^{\circ} at

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Explanation:

The values given in the problem is

ΔG° = 1.22 ×10⁵ J/mol

T = 2400 K.

R = 8.314 J mol⁻¹ K⁻¹

The Gibbs free energy should be minimum for a spontaneous reaction and equilibrium state of any reaction is spontaneous reaction. So on simplification, the thermodynamic properties of the equilibrium constant can be obtained as related to Gibbs free energy change at constant temperature.

The relation between Gibbs free energy change with equilibrium constant is ΔG° = -RT ln K

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We get,

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