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jonny [76]
3 years ago
9

Express in scientific notation. Remember, M must be a number 1 ≤ M < 10. 0.000543 =

Chemistry
2 answers:
alexandr1967 [171]3 years ago
7 0
The correct answer would be <span>5.43 x 10^-4</span>
attashe74 [19]3 years ago
3 0

Answer : The given number in scientific notation will be, 5.43\times 10^{-4}

Explanation :

Scientific notation : It is the representation of expressing the numbers that are too big or too small and are represented in the decimal form with one digit before the decimal point times 10 raise to the power.

For example :

5000 is written as 5.0\times 10^3

889.9 is written as 8.899\times 10^{-2}

As we are given that the number is, 0.000543

This number is written in scientific notation as :

5.43\times 10^{-4}

Hence, the given number in scientific notation will be, 5.43\times 10^{-4}

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N204 is the correct answer
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A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indicated partial pressures: CO2, 12
Serhud [2]

Answer:

P_{He}=219mmHg

m_{He}=0.618gHe

Explanation:

Hello,

By applying the Dalton's law, we can compute the partial pressure of the helium has:

P_{tot}=P_{CO_2}+P_{Ar}+P_{O_2}+P_{He}

Now, solving for the partial pressure of the helium gas we get:

P_{He}=P_{tot}-P_{CO_2}-P_{Ar}-P_{O_2}=745mmHg-125mmHg-214mmHg-187mmHg\\P_{He}=219mmHg=0.288atm

On the other hand, the mass of the helium gas is computed via the ideal gas equation in terms of the helium's mass:

PV=\frac{m_{He}}{M_{He}}RT\\m_{He}=\frac{M_{He}PV}{RT} =\frac{4g/mol*0.288atm*12L}{0.082\frac{atm*L}{mol*K}*273K}\\ m_{He}=0.618gHe

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7 0
3 years ago
476 nm = [? ]10<br>cm<br>give your answer in scientific notation.
KatRina [158]

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6 0
3 years ago
For the reaction N2(g) + O2(g)2NO(g) H° = 181 kJ and S° = 24.9 J/K G° would be negative at temperatures (above, below) K. Enter
12345 [234]

ΔG deg will be negative above 7.27e+3 K.

<u>Explanation:</u>

  • The ΔG deg with the temperature can be found using the formula and the formula is given below
  • ΔG deg = ΔH deg - T ΔS deg
  • Given data, ΔH deg = 181kJ and ΔSdeg=24.9J/K
  • -T ΔS deg will be always negative and ΔG deg = ΔH deg  will  be  positive and ΔG deg will be negative at relatively high temperatures and positive at relatively low temperatures
  • solving the equation and substitute  ΔGdeg=0
  • ΔGdeg = ΔHdeg - T ΔSdeg
  • T= ΔHdeg/ΔSdeg
  • T=181 kJ / 2.49e-2 kJK-1
  • By simplification we get
  • T=7.27 × 10^3 K.
  • Therefore, Go will be negative above   7.27 × 10^3 K
  • Since ΔG deg = -RT lnK, when ΔGdeg < 0, K > 1 so the reaction will have K > 1 above 7.27 × 10^3 K.
  • ΔG deg will be negative above 7.27e+3 K.

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7 0
3 years ago
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