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4 years ago

Can this reaction take place/does it exist - . CaCl2+CO2+H20----> CaCO3 + 2HCl

1 answer:

6 0

Yes the reaction given above does exist
First of all CaCl2 will react with water to form CaO and HCl then it will react with CO2 to form <span>CaCO3
</span>CaCO3 + 2HCl <span>>>></span> CaCl2+CO2+H20
so i conclude it does exist
hope it helps

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What type of bond forms when electrons are transferred (lose or gain) from one atom to another?

Zarrin [17]

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3 years ago

A student heats a sample of hydrate once, and the mass of the sample and the evaporating dish is 16.428 g. After a second heatin

jolli1 [7]

Answer:

12.371 g

Explanation:

Given :

$m_{evaporating\ dish}=1.135\ g$

$m_{evaporating\ dish}+m_{Hydrate\ sample}=25.637\ g$

$m_{evaporating\ dish}+m_{First\ heated\ sample}=16.428\ g$

$m_{evaporating\ dish}+m_{Second\ heated\ sample}=13.266\ g$

Mass of salt hydrate:

$m_{evaporating\ dish}=1.135\ g$

$m_{evaporating\ dish}+m_{Hydrate\ sample}=25.637\ g$

$m_{Hydrate\ sample}=25.637-m_{evaporating\ dish}\ g=25.637-1.135\ g=24.502\ g$

Mass of salt anhydrous:

$m_{evaporating\ dish}=1.135\ g$

$m_{evaporating\ dish}+m_{Second\ heated\ sample}=13.266\ g$

$m_{Second\ heated\ sample}=m_{salt\ anhydrous}=13.266-m_{evaporating\ dish}\ g=13.266-1.135\ g=12.131\ g$

Mass of water:

$m_{water}=m_{Hydrate\ sample}-m_{salt\ anhydrous}=24.502-12.131\ g=12.371\ g$

$m_{water}=12.371\ g$

4 0

4 years ago

You mix 125 mL of 0.170 M with 50.0 mL of 0.425 M in a coffee-cup calorimeter, and the temperature of both solutions rises from

kondaur [170]

Here is the correct question

You mix 125 mL of 0.170 M CsOH with 50.0 mL of 0.425 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 20.20 °C before mixing to 22.17 °C after the reaction. What is the enthalpy of reaction per mole of ? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g · K. Enthalpy of reaction = kJ/mol

Answer:

75.059 kJ/mol

Explanation:

The formula for calculating density is:

$density = \frac{mass}{volume}\\$

Making mass the subject of the formula; we have :

mass = density × volume

which can be rewritten as:

mass of the solution = density × volume of the solution

= 1.00 g/mL × (125+ 50 ) mL

= 175 g

Specific heat capacity = 4.2 J/g.K

∴ the energy absorbed is = mcΔT

= 175 × 4.2 × (22.17 - 20.00) ° C

= 1594.95 J

= 1.595 J

number of moles of CsOH = $\frac{125}{1000} *100$

= 0.2125 mole

Therefore; the enthalpy of the reaction = $\frac{Energy \ absorbed }{number \ of \ moles}$

= $\frac{1.595}{0.02125}$

= 75.059 kJ/mol

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3 years ago

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pashok25 [27]

Inertia is your answer

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3 years ago

What was the half-life of a new isotope?

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In order to determine the half-life of a substance, we simply use:
t(1/2) = ln(2) / λ

Where λ is the decay constant for that specific isotope.

8 0

4 years ago