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2 years ago

What is the complete ionic equation of 2AgNO3 (aq) + CaCl2(aq) ---> 2AgCl2( (aq) + 2(NO3 )Ca

Chemistry

1 answer:

irinina [24]2 years ago

8 0

Answer:2Ag+ + 2NO3- + Ca++ + 2Cl- —> 2Ag+ + 2Cl- + 2NO3- + Ca++

Explanation:

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A 41.1 g sample of solid CO2 (dry ice) is added to a container at a temperature of 100 K with a volume of 3.4 L.A. If the contai

marta [7]

Answer:

Approximately 6.81 × 10⁵ Pa.

Assumption: carbon dioxide behaves like an ideal gas.

Explanation:

Look up the relative atomic mass of carbon and oxygen on a modern periodic table:

C: 12.011;
O: 15.999.

Calculate the molar mass of carbon dioxide $\rm CO_2$ :

$M\!\left(\mathrm{CO_2}\right) = 12.011 + 2\times 15.999 = 44.009\; \rm g \cdot mol^{-1}$ .

Find the number of moles of molecules in that $41.1\;\rm g$ sample of $\rm CO_2$ :

$n = \dfrac{m}{M} = \dfrac{41.1}{44.009} \approx 0.933900\; \rm mol$ .

If carbon dioxide behaves like an ideal gas, it should satisfy the ideal gas equation when it is inside a container:

$P \cdot V = n \cdot R \cdot T$ ,

where

$P$ is the pressure inside the container.
$V$ is the volume of the container.
$n$ is the number of moles of particles (molecules, or atoms in case of noble gases) in the gas.
$R$ is the ideal gas constant.
$T$ is the absolute temperature of the gas.

Rearrange the equation to find an expression for $P$ , the pressure inside the container.

$\displaystyle P = \frac{n \cdot R \cdot T}{V}$ .

Look up the ideal gas constant in the appropriate units.

$R = 8.314 \times 10^3\; \rm L \cdot Pa \cdot K^{-1} \cdot mol^{-1}$ .

Evaluate the expression for $P$ :

$\begin{aligned} P &=\rm \frac{0.933900\; mol \times 8.314 \times 10^3 \; L \cdot Pa \cdot K^{-1} \cdot mol^{-1} \times 298\; K}{3.4\; L} \cr &\approx \rm 6.81\times 10^5\; Pa \end{aligned}$ .

Apply dimensional analysis to verify the unit of pressure.

4 0

3 years ago

When the particles of a gas decrease in energy what happens?

NeTakaya

It changes to a liquid

3 0

3 years ago

Read 2 more answers

The osmolarity of a 1-l bottle of 5% dextrose solution is _____ mosm/l.

Pachacha [2.7K]

M(dextrose) = 50 g.
V(solution) = 1 L.
n(dextrose) = 50 g ÷ 180 g/mol.
n(dextrose) = 0,27 mol.
Osmotic concentration (osmolarity) is a measure of how many osmoles of particles of solute it contains per liter.
The osmolarity = n(dextrose) ÷ V(solution).
The osmolarity = 0,27 mol ÷ 1 L.
The osmolarity = 0,27 mol/L · 1000 mmol/m.
The osmolarity (dextrose) = 270 mosm/L.
The osmolarity (dextrose monohydrate) = 50 g÷197 g/mol·1000 =254mosm/L

7 0

3 years ago

Read 2 more answers

The number of electrons in a neutral atom of hydrogen (H) atom is

vesna_86 [32]

There is one electron

7 0

3 years ago

Calculate the number of miles of NH4SO4 in 250 ml of a 1.5 M solution

ahrayia [7]

I’m guessing you mean moles. So the big M stands for mol/L. That means first you’d want to convert your mL to L. To do this write your 250mL then make parenthesis for the conversion. 1L=1000mL
250mL(1L/1000mL). Since the mL is on the bottom in the parenthesis we can cancel them out. Now all we do is divide and keep the L.
.250L is what you get. Now we need to figure out how to cancel the L with what we have left. We know M stands for Moles/L so this means in order to get ride of L we need to multiply our new number times the 1.5
.250L X 1.5 moles
_______

1L
This gives us 0.375 moles NH4SO4

3 0

3 years ago