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2 years ago

Is the prime meridian a longitudinal or latitudinal line?

Chemistry

1 answer:

Nesterboy [21]2 years ago

4 0

Answer:

longitudinal

Explanation:

A prime meridian is the meridian (a line of longitude) in a geographic coordinate system at which longitude is defined to be 0°. Together, a prime meridian and its anti-meridian (the 180th meridian in a 360°-system) form a great circle. This great circle divides a spheroid into two hemispheres.

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Calculate to three significant digits the density of dinitrogen monoxide gas at exactly and exactly . You can assume dinitrogen

Ulleksa [173]

Answer:

see explanation below

Explanation:

You miss the part of the temperature and pressure. According to what I found this is held under 30 °C (or 303 K) and 1 atm.

The problem states that we can treat this gas as an ideal gas, therefore, we can use the equation of an ideal gas which is:

PV = nRT (1)

Now, the density (d) is calculated as:

d = m/V (2)

We can rewrite (2) in function of mass of volume so:

m = d*V (3)

Now, the moles (n) of (1) can be calculated like this:

n = m /MM (4)

If we replace it in (1) and then, (3) into this we have the following:

PV = mRT/MM ----> replacing (3):

PV = dVRT/MM ----> V cancels out so finallly:

P = dRT/MM

d = P * MM / RT (5)

The molar mass of N2O is 44 g/mol So, replacing all the data we have:

d = 1 * 44 / 0.082 * 303

d = 1.77 g/L

5 0

2 years ago

Which has the smallest electronegativity? a Calcium b Argon c Hydrogen d Bromine

Mademuasel [1]

Answer: Calcium

Explanation:

Calcium has only one electronegativity.

4 0

2 years ago

Theoretically, what mass of [Co(NH3)4(H2O)2]Cl2 could be produced from 4.00 g of CoCl2•6H2O starting material. If 1.20 g of [Co(

Romashka [77]

<u>Answer:</u> The theoretical yield and percent yield of $[Co(NH_3)_4(H_2O)_2]Cl_2$ is 3.93 g and 30.53 % respectively

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of $CoCl_2.6H_2O$ = 4.00 g

Molar mass of $CoCl_2.6H_2O$ = 238 g/mol

Putting values in equation 1, we get:

$\text{Moles of }CoCl_2.6H_2O=\frac{4.00g}{238g/mol}=0.0168mol$

The chemical equation for the reaction of $CoCl_2.6H_2O$ to form $[Co(NH_3)_4(H_2O)_2]Cl_2$ follows:

$CoCl_2.6H_2O+4NH_3\rightarrow [Co(NH_3)_4(H_2O)_2]Cl_2+4H_2O$

By Stoichiometry of the reaction:

1 mole of $CoCl_2.6H_2O$ produces 1 mole of $[Co(NH_3)_4(H_2O)_2]Cl_2$

So, 0.0168 moles of $CoCl_2.6H_2O$ will produce = $\frac{1}{1}\times 0.0168=0.0168mol$ of $[Co(NH_3)_4(H_2O)_2]Cl_2$

Now, calculating the mass of $[Co(NH_3)_4(H_2O)_2]Cl_2$ from equation 1, we get:

Molar mass of $[Co(NH_3)_4(H_2O)_2]Cl_2$ = 234 g/mol

Moles of $[Co(NH_3)_4(H_2O)_2]Cl_2$ = 0.0168 moles

Putting values in equation 1, we get:

$0.0168mol=\frac{\text{Mass of }[Co(NH_3)_4(H_2O)_2]Cl_2}{234g/mol}\\\\\text{Mass of }[Co(NH_3)_4(H_2O)_2]Cl_2=(0.0168mol\times 234g/mol)=3.93g$

To calculate the percentage yield of $[Co(NH_3)_4(H_2O)_2]Cl_2$ , we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of $[Co(NH_3)_4(H_2O)_2]Cl_2$ = 1.20 g

Theoretical yield of $[Co(NH_3)_4(H_2O)_2]Cl_2$ = 3.93 g

Putting values in above equation, we get:

$\%\text{ yield of }[Co(NH_3)_4(H_2O)_2]Cl_2=\frac{1.20g}{3.93g}\times 100\\\\\% \text{yield of }[Co(NH_3)_4(H_2O)_2]Cl_2=30.53\%$

Hence, the theoretical yield and percent yield of $[Co(NH_3)_4(H_2O)_2]Cl_2$ is 3.93 g and 30.53 % respectively

6 0

2 years ago

What is boiling point

klasskru [66]

Answer:

The temperature at which the given substance starts to boil is called boiling point.

I HOPE IT HELPED U

STAY SAFE STAY HAPPY

5 0

2 years ago

Read 2 more answers

Calculate the concentration of the following solution in mol/dm3 0.1 moles of NaCl in 200 cm3

taurus [48]

1 $cm ^{3}$ = 0.001 $dm ^{3}$ . Therefore 200 $cm ^{3}$ = 0.2 $dm ^{3}$ . Molarity = $\frac{number of moles of NaCl}{volume of the solution} = \frac{0.1}{0.2} = 0.5 mol/dm^{3}$ . Hope this helps.

8 0

2 years ago