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Ierofanga [76]
4 years ago
9

PLEASE HELPP!!!!

Chemistry
1 answer:
Natasha_Volkova [10]4 years ago
4 0

Answer:

<em>The combined law is:</em>

          \dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}

See the derivation below.

Explanation:

<em><u>1. Boyle's law:</u></em>

    PV=constant\\\\P_1V_1=P_2V_2

<em />

<u><em>2. Charles' law:</em></u>

        \dfrac{V}{T}=constant\\\\\\\dfrac{V_1}{T_1}=\dfrac{V_2}{T_2}

<em><u>3. Gay-Lussac’s law</u></em>

      \dfrac{P}{T}=constant\\\\\\\dfrac{P_1}{T_1}=\dfrac{P_2}{T_2}

<u>4. Summary:</u>

  •    PV = K
  •    V/T = K'
  •    P/T = K''

Mulitply PV by V/T and P/T

        PV\times \dfrac{V}{T}\times \dfrac{P}{T}=K\times K'\times K''\\\\\\\dfrac{P^2V^2}{T^2}=constant\\\\\\\sqrt{\dfrac{P^2V^2}{T^2}}=\sqrt{constant}\\\\\\\dfrac{PV}{T}=constant

Thus:

          \dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}

Which is<em> the combined law.</em>

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What is the percent yield for a chemical reaction if the actual yield is 36 g and the theorical yield is 45 g.
SpyIntel [72]

Answer:

⇒ Percent yield = 80 %

Explanation:

Given:

Actual yield = 36 g

Theoretical yield = 45 g

Find:

Percent yield

Computation:

⇒ Percent yield = [Actual yield / Theoretical yield] 100%

⇒ Percent yield = [36 / 45] 100%

⇒ Percent yield =[0.8] 100%

⇒ Percent yield = 80 %

4 0
3 years ago
A 37.2 g sample of copper at 99.8 °C is carefully placed into an insulated container containing 188 g of water at 18.5 °C. Calcu
klasskru [66]

Answer:

T₂ = 19.95°C

Explanation:

From the law of conservation of energy:

Heat\ Lost\ by\ Copper = Heat\ Gained\ by\ Water\\m_cC_c\Delta T_c = m_wC_w\Delta T_w

where,

mc = mass of copper = 37.2 g

Cc = specific heat of copper = 0.385 J/g.°C

mw = mass of water = 188 g

Cw = specific heat of water = 4.184 J/g.°C

ΔTc = Change in temperature of copper = 99.8°C - T₂

ΔTw = Change in temperature of water = T₂ - 18.5°C

T₂ = Final Temperature at Equilibrium = ?

Therefore,

(37.2\ g)(0.385\ J/g.^oC)(99.8\ ^oC-T_2)=(188\ g)(4.184\ J/g.^oC)(T_2-18.5\ ^oC)\\99.8\ ^oC-T_2 = \frac{(188\ g)(4.184\ J/g.^oC)}{(37.2\ g)(0.385\ J/g.^oC)}(T_2-18.5\ ^oC)\\\\99.8\ ^oC-T_2 = (54.92) (T_2-18.5\ ^oC)\\54.92T_2+T_2 = 99.8\ ^oC + 1016.02\ ^oC\\\\T_2 = \frac{1115.82\ ^oC}{55.92}

<u>T₂ = 19.95°C</u>

6 0
3 years ago
E=hv h= 6.62 x 10^-34 m^2 kg/ s
Drupady [299]

v=5.0×10^12Hz

\\ \sf\longmapsto E=hv

\\ \sf\longmapsto E=6.626\times 10^{-34}Js\times 5\times 10^12s^{-1}

\\ \sf\longmapsto E=33.13\times 10^{-22}J

7 0
3 years ago
How many grams is 2.393 x 10^24 atoms of CI
Iteru [2.4K]

Answer:

There are 140.9 grams in 2.393*10²⁴ aotms of Cl.

Explanation:

Avogadro's Number or Avogadro's Constant is called the number of particles that make up a substance (usually atoms or molecules) and that can be found in the amount of one mole of said substance. Its value is 6.023*10²³ particles per mole. Avogadro's number represents a quantity without an associated physical dimension, so it is considered a pure number that allows describing a physical characteristic without an explicit dimension or unit of expression. Avogadro's number applies to any substance.

Then you can apply the following rule of three: if 6.023*10²³ atoms are contained in 1 mole of the compound, 2.393*10²⁴ atoms are contained in how many moles?

amount of moles=\frac{2.393*10^{24} *1 mole}{6.023*10^{23} }

amount of moles= 3.973

If the molar mass of Cl is 35.453 \frac{g}{mole}, then the amount of mass that contains 3.973 moles can be calculated as:

3.973 moles*35.453 \frac{g}{mole}= 140.85 grams ≅ 140.9 grams

<u><em>There are 140.9 grams in 2.393*10²⁴ aotms of Cl.</em></u>

7 0
3 years ago
Which statement about hydrogen bonding is true? Select one:
Alexandra [31]

Answer:

E.

Explanation:

All answers other than E have the incorrect bonding capabilities or other incorrect information.

8 0
4 years ago
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