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3 years ago

How much heat would be released by 1.3 kg of water if it's temperature went from 295 k to 274 k

Chemistry

1 answer:

kicyunya [14]3 years ago

4 0

Answer: The energy released will be 114.223 kJ.

Explanation:

To calculate the amount of heat released, we use the formula:

$Q= m\times c\times \Delta T$

Q = heat gained or released

m = mass of the substance = 1.3kg = 1300 g (Conversion factor: 1kg = 1000g)

c = heat capacity of water = 4.184 J/g K

$\Delta T={\text{Change in temperature}}=(274-295)K=-21K$

Putting values in above equation, we get:

$Q=1300g\times 4.184J/gK\times (-21)K$

Q = -114223 Joules = -114.223 kJ (Conversion Factor: 1kJ = 1000J)

Negative sign implies heat released.

Hence, heat released by 1.3 kg of water is 114.223kJ.

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Calculate the energy (in J/atom) for vacancy formation in silver, given that the equilibrium number of vacancies at 800 C is 3.6

MAXImum [283]

Answer:

the energy vacancies for formation in silver is $\mathbf{Q_v = 3.069*10^{-4} \ J/atom}$

Explanation:

Given that:

the equilibrium number of vacancies at 800 °C

i.e T = 800°C is 3.6 x 10¹⁷ cm3

Atomic weight of sliver = 107.9 g/mol

Density of silver = 9.5 g/cm³

Let's first determine the number of atoms in silver

Let silver be represented by N

SO;

$N = \dfrac{N_A* \rho _{Ag}}{A_{Ag}}$

where ;

$N_A =$ avogadro's number = $6.023*10^{23} \ atoms/mol$

$\rho _{Ag}$ = Density of silver = 9.5 g/cm³

$A_{Ag}$ = Atomic weight of sliver = 107.9 g/mol

$N = \dfrac{(6.023*10^{23} \ atoms/mol)*( 9.5 \ g/cm^3)}{(107.9 \ g/mol)}$

N = 5.30 × 10²⁸ atoms/m³

However;

The equation for equilibrium number of vacancies can be represented by the equation:

$N_v = N \ e^{^{-\dfrac{Q_v}{KT}}$

From above; Considering the natural logarithm on both sides; we have:

$In \ N_v =In N - \dfrac{Q_v}{KT}$

Making $Q_v$ the subject of the formula; we have:

${Q_v = - {KT} In( \dfrac{ \ N_v }{ N})$

where;

K = Boltzmann constant = 8.62 × 10⁻⁵ eV/atom .K

Temperature T = 800 °C = (800+ 273) K = 1073 K

$Q _v =-( 8.62*10^{-5} \ eV/atom.K * 1073 \ K) \ In( \dfrac{3.6*10^{17}}{5.3 0*10^{28}})$

$\mathbf{Q_v = 2.38 \ eV/atom}$

Where;

1 eV = 1.602176565 × 10⁻¹⁹ J

Then

$Q_v = (2.38 \ * 1.602176565 * 10^{-19} ) J/atom }$

$\mathbf{Q_v = 3.069*10^{-4} \ J/atom}$

Thus, the energy vacancies for formation in silver is $\mathbf{Q_v = 3.069*10^{-4} \ J/atom}$

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3 years ago

When a lithium atom forms an Li+ ion, the lithium atom

gizmo_the_mogwai [7]

4, loses an electron. a plus sign indicates an atom is losing an electron while a minus sign indicates an atom is gaining an electron
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lora16 [44]

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GaryK [48]

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3 years ago