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3 years ago

What is the formula of a compound formed between iodine (I) and calcium (Ca)?

Chemistry

2 answers:

bixtya [17]3 years ago

8 0

Answer: The chemical formula for the compound will be $CaI_2$

Explanation:

Calcium is the 20th element of the periodic table having electronic configuration of $[Ar]4s^2$

This element will loose 2 electrons and thus shows an oxidation state of +2 units.

Iodine is the 53rd element of the periodic table having electronic configuration of $[Kr]5s^24d^{10}5p^5$

This element requires 1 electron and thus shows an oxidation state of -1 units.

So, by criss-cross method, the oxidation state of the ions will get exchanged and they form the subscripts of the other ions. This results in the formation of a neutral compound.

Hence, the chemical formula for the compound formed will be $CaI_2$

Nadya [2.5K]3 years ago

7 0

Calcium iodide (chemical formula CaI2)

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Consider the first-order reaction described by the equation At a certain temperature, the rate constant for this reaction is 5.8

zubka84 [21]

Answer: The half life of the reaction is 1190.7 seconds

Explanation:

The equation used to calculate rate constant from given half life for first order kinetics:

$t_{1/2}=\frac{0.693}{k}$

where,

k = rate constant of the reaction = $5.82\times 10^{-4}s^{-1}$

$t_{1/2}$ = half life of the reaction = ?

Putting values in above equation, we get:

$t_{1/2}=\frac{0.693}{5.82\times 10^{-4}s^{-1}}=1190.7s$

Hence, the half life of the reaction is 1190.7 seconds

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3 years ago

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sergejj [24]

Answer:

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Explanation:

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Artyom0805 [142]

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16.25 g of water at 54 C relaeases 402.7 J. What will be its final temp?

leonid [27]

Data:
Q = 402.7 J → releases → Q = - 402.7 J
m = 16.25 g
T initial = 54 ºC
adopting: c = 4.184J/g/°C
ΔT (T final - T initial) = ?

Solving:

Q = m*c*ΔT
-402.7 = 16.25*4.184*ΔT
-402.7 = 67.99*ΔT
$\Delta\:T = \frac{-402.7}{67.99}$
$\boxed{\Delta\:T \approx -5.92\:^0C}$

If: ΔT (T final - T initial) = ?
$-5.92^0 = T_{final} - 54^0$
$T_{final} = 54^0 - 5.92^0$
$\boxed{\boxed{T_{final} = 48.08\:^0C}}\end{array}}\qquad\quad\checkmark$

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4 years ago