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Kay [80]
3 years ago
15

Why does it take less

Chemistry
1 answer:
KengaRu [80]3 years ago
8 0

Answer:I’m not for sure

Explanation:

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If 12.5 grams of the original sample of cesium-137 remained after 90.6 years, what was the mass of the original sample?
myrzilka [38]

Answer:

Mass of original sample = 100 g

Explanation:

Half life of cesium-137 = 30.17 years

t_{1/2}=\frac {ln\ 2}{k}

Where, k is rate constant

So,  

k=\frac{\ln2}{t_{1/2}}

k=\frac{\ln2}{30.17}\ year^{-1}

The rate constant, k = 0.02297 year⁻¹

Time = 90.6 years

Using integrated rate law for first order kinetics as:

[A_t]=[A_0]e^{-kt}

Where,  

[A_t] is the concentration at time t

[A_0] is the initial concentration

Initial concentration [A_0] = ?

Final concentration [A_t] = 12.5 grams

Applying in the above equation, we get that:-

12.5\ g=[A_0]e^{-0.02297\times 90.6}

[A_0]=\frac{12.5}{e^{-0.02297\times 90.6}}\ g=100\ g

<u>Mass of original sample = 100 g</u>

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3 years ago
The Toucan has a long, narrow beak that allows it to reach fruit that is hard to reach for other birds. Plants, like the Monster
gladu [14]
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2 years ago
Will Mark Brainliest <br>Aswer for<br>box 1 and box 2<br>On top of the oval says <br>A-U-G-G-C-A
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How does Kinetic energy and how does it relates to diffusion and temperature.
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3 years ago
Consider the reaction FeO (S) + CO(g) &lt;-----&gt; Fe(s) + CO2(g) for which KP is found to have the following values:
Svetach [21]

Explanation:

\Delta G^o=-RT\ln K_1

where,

R = Gas constant = 8.314J/K mol

T = temperature = 600^oC=[273.15+600]K=873.15 K

K_p = equilibrium constant at 600°C =  0.900

Putting values in above equation, we get:

\Delta G^o=-(8.314J/Kmol)\times 873.15 K\times \ln (0.900 )

\Delta G^o=764.85 J/mol

The ΔG° of the reaction at 764.85 J/mol is 764.85 J/mol.

Equilibrium constant at 600°C = K_1=0.900

Equilibrium constant at 1000°C = K_2=0.396

T_1=[273.15+600]K=873.15 K

T_2=[273.15+1000]K=1273.15 K

\ln \frac{K_2}{K_1}=\frac{\Delta H^o}{R}\times [\frac{1}{T_1}-\frac{1}{T_2}]

\ln \frac{0.396}{0.900}=\frac{\Delta H^o}{8.314 J/mol K}\times [\frac{1}{873.15 K}-\frac{1}{1273.15 K}]

\Delta H^o=-18,969.30 J/mol

The ΔH° of the reaction at 600 C is -18,969.30 J/mol.

ΔG° = ΔH° - TΔS°

764.85 J/mol = -18,969.30 J/mol - 873.15 K × ΔS°

ΔS° = -22.60 J/K mol

The ΔS° of the reaction at 600 C is -22.60 J/K mol.

FeO (s) + CO(g)\rightleftharpoons Fe(s) + CO_2(g)

Partial pressure of carbon dioxide = p_1=P\times \chi_1

Partial pressure of carbon monoxide = p_2=P\times \chi_2

Where \chi_1\& \chi_2 mole fraction of carbon dioxide and carbon monoxide gas.

The expression of K_p is given by:

K_p=\frac{p_1}{p_2}=\frac{P\times \chi_1}{P\times \chi_2}

0.900=\frac{\chi_1}{\chi_2}

\chi_1=0.900\times \chi_2

\chi_1+\chi_2=1

0.9\chi_2+\chi_2=1

1.9\chi_2=1

\chi_2=\frac{1}{1.9}=0.526

\chi_1=1-\chi_2=1-0.526=0.474

Mole fraction of carbon dioxide at 600°C is 0.474.

6 0
3 years ago
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