Fe-C-Cr alloy is covalent or ionic?

Which is an example of a medicine that is made up of synthetic materials?

iren [92.7K]

Answer: Aspirin

Explanation:

6 0

3 years ago

Which statements correctly describe the human skeletal system?

zhenek [66]

Answer:

A

Explanation:

Well, the human skeletal system produce red blood cells into and for the body.

4 0

3 years ago

What isotope has 13 protons and 14 neutrons? Enter the name of the element followed by a hyphen and the mass number (e.g., urani

Lilit [14]

Answer: The element is represented as Aluminium-27

Explanation:

Atomic number is defined as the number of protons or number of electrons that are present in an electrically neutral atom.

Atomic number = Number of electrons = Number of protons = 13

Mass number is defined as the sum of number of protons and neutrons that are present in an atom.

Mass number = Number of protons + Number of neutrons = 13 + 14 = 27

Thus the element with atomic number of 13 is aluminium and its mass number is 27. Thus it is represented as Aluminium-27

5 0

4 years ago

Calculate the maximum solubility of silver carbonate, Ag2CO3 in g/L when in the presence of 0.057 M AgNO3. The solubility produc

Andreyy89

Answer:

Approximately $4.2 \times 10^{-7}\; \rm g \cdot L^{-1}$ .

Explanation:

Start by finding the concentration of $\rm Ag_2CO_3$ at equilibrium. The solubility equilibrium for

$\rm Ag_2CO_3 \; (s) \rightleftharpoons 2\, Ag^{+}\; (aq) + {CO_3}^{2-}\; (aq)$ .

The ratio between the coefficient of $\rm Ag_2CO_3$ and that of $\rm Ag^{+}$ is $1:2$ . For

Let the increase in $\rm {CO_3}^{2-}$ concentration be $+x\; \rm mol \cdot L^{-1}$ . The increase in $\rm Ag^{+}$ concentration would be $+2\,x\; \rm mol \cdot L^{-1}$ . Note, that because of the $0.057\; \rm mol \cdot L^{-1}$ of $\rm AgNO_3$ , the concentration of

The concentration of $\rm Ag^{+}$ would be $(0.057 + 2\, x) \; \rm mol\cdot L^{-1}$ .
The concentration of $\rm {CO_3}^{2-}$ would be $x\; \rm mol \cdot L^{-1}$ .

Apply the solubility product expression (again, note that in the equilibrium, the coefficient of $\rm Ag^{+}$ is two) to obtain:

$\begin{aligned}&\rm \left[Ag^{+}\right]^2 \cdot \left[{CO_3}^{2-}\right] = K_{\text{sp}} \\ & \implies (0.057 + x)^2\cdot x = 8.1 \times 10^{-12} \end{aligned}$ .

Note, that the solubility product of $\rm Ag_2CO_3$ , $K_{\text{sp}} = 8.1 \times 10^{-12}$ is considerably small. Therefore, at equilibrium, the concentration of

Apply this approximation to simplify $(0.057 + x)^2\cdot x = 8.1 \times 10^{-12}$ :

$0.057^2\, x \approx (0.057 + x)^2 \cdot x = 8.1 \times 10^{-12}$ .

$\begin{aligned} x &\approx \frac{8.1 \times 10^{-12}}{0.057^2}\end{aligned}$ .

Calculate solubility (in grams per liter solution) from the concentration. The concentration of $\rm Ag_2CO_3$ is approximately $\displaystyle \frac{8.1 \times 10^{-12}}{0.057^2}\; \rm mol\cdot L^{-1}$ , meaning that there are approximately $\displaystyle n = \frac{8.1 \times 10^{-12}}{0.057^2}\; \rm mol$ of

$\begin{aligned}m &= n \cdot M \\ &\approx \displaystyle \frac{8.1 \times 10^{-12}}{0.057^2} \; \rm mol\times 167.91\; g \cdot mol^{-1} \\ &\approx 4.2 \times 10^{-7}\; \rm g \end{aligned}$ .

As a result, the maximum solubility of $\rm Ag_2CO_3$ in this solution would be approximately $4.2 \times 10^{-7}\; \rm g \cdot L^{-1}$ .

8 0

3 years ago

The molecular weight of H 2 SO 4 is:<br><br> 49.078 g/mole<br> 98.086 g/mole<br> 194.296 g/mole

romanna [79]

Answer:

the molecular weight of H2SO4 is 98.086g/mole

8 0

4 years ago