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Paul [167]
3 years ago
14

In which position are the earth, moon, and sun during a new moon?

Chemistry
1 answer:
RSB [31]3 years ago
4 0

Answer:

They are in this position

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What is the % Yield if 3.8 g of Cu was produced?
seraphim [82]
83.9 is the answer i’m pretty sure
3 0
3 years ago
What factors affect the speed of a wave? Check all that apply. the amplitude of the wave the energy of the wave the temperature
Lena [83]

Answer:

I believe its 1,2, and 5

Explanation:

4 0
3 years ago
(a) Given that Ka for acetic acid is 1.8 X 10^-5 and that for hypochlorous acid is 3.0 X 10^-8, which is the stronger acid? (b)
Gala2k [10]

Answer:

HOAc is stronger acid than HClO

ClO⁻ is stronger conjugate base than OAc⁻

Kb(OAc⁻) = 5.5 x 10⁻¹⁰

Kb(ClO⁻) = 3.3 x 10⁻⁷

Explanation:

Assume 0.10M HOAc => H⁺ + OAc⁻  with Ka = 1.8 x 10⁻⁵

=> [H⁺] = √Ka·[Acid] =√(1.8 x 10⁻⁵)(0.10) M = 1.3 x 10⁻³M H⁺

Assume 0.10M HClO => H⁺ + ClO⁻ with Ka = 3 x 10⁻⁸

=> [H⁺] = √(3 x 10⁻⁸)(0.10)M = 5.47 x 10⁻⁵M H⁺

HOAc delivers more H⁺ than HClO and is more acidic.

Kb = Kw/Ka, Kw = 1 x 10⁻¹⁴

Kb(OAc⁻) = 5.5 x 10⁻¹⁰

Kb(ClO⁻) = 3.3 x 10⁻⁷

4 0
3 years ago
Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation:
egoroff_w [7]

The grams  of  oxygen that are required  to produce 1  mole  of H₂O  is 16 g ( answer  B)

<u><em> calculation</em></u>

2 CH₄  + 2NH₃ +3 O₂ → 2HCN  + 6H₂O

step 1: use the mole ratio to find moles of O₂

from equation above the  mole ratio  of O₂: H₂O  is 3:6 therefore the moles of O₂  = 1 mole x3/6 =0.5 moles

step  2: find   mass of O₂

mass= moles x molar mass

from periodic table the molar mass  of O₂ = 16 x2= 32 g/mol

mass O₂ = 0.5 moles x 32 g/mol = 16 g (answer B)

6 0
3 years ago
Read 2 more answers
Jacob floated a long steel sewing needle on a small piece of cork in a glass of water. He noticed that as he turned the glass ar
max2010maxim [7]

Answer:

<em>Hello, Your answer will be </em><em>B) Jacob's backyard is on the north side of his house.</em>

<em>Hope That Helps!</em>

7 0
2 years ago
Read 2 more answers
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