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ella [17]
3 years ago
12

Take an ice cube at -196 °C and drop it into an ice-water mixture at 0 °C and wait. The ice cube warms up so E_thermal of the ic

e cube increased.
What energy system decreased?
Chemistry
1 answer:
ser-zykov [4K]3 years ago
5 0

Answer:

Bond energy system will decrease.

Explanation:

When ice cube at -196 °C is dropped into ice-water at 0 °C then the heat energy transfers from ice-water to ice cube (since, heat energy always transfers from a hot body to cold body, according to the second law of thermodynamics). This transfer of heat energy into the ice cube increases the thermal energy of the ice cube however, the increase in thermal energy, weakens the bonds between atoms in the ice cube and changes the physical state of the ice cube thereby, results in the decrease in bond energy system.  

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Which of the Atoms shown has an atomic number four
dimulka [17.4K]

Answer:

B

Explanation:

Atomic # = Protons

it says 4 p in the inside of the orbital

4 0
3 years ago
Radioactive decay can be described by the following equation where is the original amount of the substance, is the amount of the
soldi70 [24.7K]

Answer:

Iron remains = 17.49 mg

Explanation:

Half life of iron -55 = 2.737 years (Source)

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

Where, k is rate constant

So,  

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

k=\frac {ln\ 2}{2.737}\ year^{-1}

The rate constant, k = 0.2533 year⁻¹

Time = 2.41 years

[A_0] = 32.2 mg

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

So,  

[A_t]=32.2\times e^{-0.2533\times 2.41}\ mg

[A_t]=32.2\times e^{-0.610453}\ mg

[A_t]=17.49\ mg

<u>Iron remains = 17.49 mg</u>

8 0
3 years ago
How many atoms of Sn are in 0.796 moles of this element?
garik1379 [7]

Answer:

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Explanation:

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3 0
3 years ago
Calculate the mass of 6 moles of H2O
RUDIKE [14]
<span>6mole of H2O contains 18×6 g=108 g</span>
8 0
3 years ago
Read 2 more answers
Determine the specific heat of copper from the fact that 38 g of 80°C copper are needed to raise the temperature of 15 g of wate
mars1129 [50]
From the equation q=mCΔT, set the q of copper = to q of water,

So --- mCΔT(copper)=mCΔT(water).

mass (Cu - copper) = 38g
mass (H2O - water) = 15g
C (H2O) = 4.184 J/g*C
ΔΤ (H2O) = 33-22 = 11*C
ΔΤ (Cu) = 33-80 = -47*C (the final temp is the same for both materials - thermal equilibrium)
C (Cu) = ?

So --- 38(-47)C[Cu]=15(4.184)(11)
     --- C[Cu]=690.36/(-1786) = 0.3865 J/g*C, or 0.39 in 2 sig figs. (The negative goes away, because specific heats are usually positive)
5 0
3 years ago
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