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3 years ago

PLEASe help. How many ions? With picture.

Chemistry

1 answer:

Likurg_2 [28]3 years ago

5 0

Since this equation is balanced, we know that the law of conversation of mass id applied, and we could calculate easily.

Na= 2
NO3= 2
Ca= 1
Cl= 1

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2. What mass of sodium chloride is produced when chlorine gas reacts with 2.29 grams of sodium iodide? The unbalanced equation i

Damm [24]

Answer:

0.88g

Explanation:

The reaction equation:

2NaI + Cl₂ → 2NaCl + I₂

Given parameters:

Mass of Sodium iodide = 2.29g

Unknown:

Mass of NaCl = ?

Solution:

To solve this problem, we work from the known to the unknown.

First find the number of NaI from the mass given;

Number of moles = $\frac{mass}{molar mass}$

Molar mass of NaI = 23 + 126.9 = 149.9g/mol

Now insert the parameters and solve;

Number of moles = $\frac{2.29}{149.9}$ = 0.015mol

So;

From the balanced reaction equation;

2 moles of NaI produced 2 moles of NaCl

0.015mole of NaI will produce 0.015mole of NaCl

Therefore;

Mass = number of moles x molar mass

Molar mass of NaCl = 23 + 35.5 = 58.5g/mol

Now;

Mass of NaCl = 0.015 x 58.5 = 0.88g

8 0

2 years ago

Dihydrogen monoxide is a(n) ____. A. covalent compound B. molecular formula C. empirical formula D. Ionic compound

olga_2 [115]

Answer:

D. Ionic compound

Explanation:

Just based on my opinion

Correct me if I'm wrong tnx:<

8 0

2 years ago

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

Question in pic please see questions below !!!

ira [324]

Answer:

its the same thing as 3 x3 or 3+3 it always come´s back as 9 or 6 Because of life

Explanation:

4 0

2 years ago

At what temperature will 0.0705 mol of Cl2 exert a pressure of 900. torr at a volume of 0.750L?

kompoz [17]

Answer:

It will exert the pressure at a temperature of 153.44 K

Explanation:

To answer this question, we shall be using the ideal gas equation;

PV = nRT

Since we are calculating the temperature, it can be made the subject of the formula.

Thus, this can be T = PV/nR

where P is the pressure = 900 torr

V is the volume = 0.75 L

n is the number of moles = 0.0705 mol

R is the molar gas constant = 62.4 L.Torr. $k^{-1}$ . $mol^{-1}$

Plugging these values into the equation, we have;

T = (900 × 0.75)/(0.0705 × 62.4)

T = 153.44 K

8 0

3 years ago