Answer:
4.92 grams of sodium phosphate (Na₃PO₄) are required to make 125 milliliters of a 0.240 M.
Explanation:
Molarity is a measure of concentration that indicates the number of moles of solute that are dissolved in a given volume.
The molarity of a solution is calculated by dividing the moles of the solute by the volume of the solution:
Molarity is expressed in units
.
In this case:
- Molarity= 0.240 M
- number of moles= ?
- volume= 125 mL= 0.125 L
Replacing in the definition of molarity:
![0.240 M=\frac{number of moles}{0.125 L}](https://tex.z-dn.net/?f=0.240%20M%3D%5Cfrac%7Bnumber%20of%20moles%7D%7B0.125%20L%7D)
Solving:
number of moles= 0.240 M*0.125 L
number of moles= 0.03 moles
Being the molar mass of sodium phosphate 164 g/mole, that is, the mass of one mole of the compound, you can calculate the mass of 0.03 moles using the following rule of three: if 1 mole of the compound has 164 grams, 0.03 moles contains how much mass?
![mass=\frac{0.03 moles*164 grams}{1 mole}](https://tex.z-dn.net/?f=mass%3D%5Cfrac%7B0.03%20moles%2A164%20grams%7D%7B1%20mole%7D)
mass= 4.92 grams
<u><em>4.92 grams of sodium phosphate (Na₃PO₄) are required to make 125 milliliters of a 0.240 M.</em></u>
Answer:
<h2>both of them</h2>
Explanation:
<h3>I hope it's helpful for you ✌</h3>
U didn’t put a picture buts a cloud that falls
Its phosphorus (P)In writing the electron configuration for Phosphorus the first two electrons will go in the 1s orbital. Since 1s can only hold two electrons the next 2 electrons for Phosphorous go in the 2s orbital. The next six electrons will go in the 2p orbital. The p orbital can hold up to six electrons. We'll put six in the 2p orbital and then put the next two electrons in the 3s. Since the 3s if now full we'll move to the 3p where we'll place the remaining three electrons. Therefore the Phosphorus electron configuration will be 1s22s22p63s23p3.
Answer:
n = 0.594 mol
Explanation:
Parameters of the question.
Heat = 979J
Initial Temperature (T1) = 10.6 C = 283.6 K (converting to Kelvin by adding 273)
FinalTemperature (T2) = 26.4 C = 299.4 K (converting to Kelvin by adding 273)
ΔT = T2 -T1 = 299.4 - 283.6 = 15.8K
Work done (W) = 221 J
number of moles (n) = ?
Formular to be used;
W=PΔV
From ideal gas equation,
PV = nRT
PΔV = nRΔT
where R = gas constant = 8.314 J / mol·K
Sunstituting in the work done equation,
we have W=nRΔT
Making n subject of formular,
![n = \frac{RT}{W}](https://tex.z-dn.net/?f=n%20%3D%20%5Cfrac%7BRT%7D%7BW%7D)
n = [8.314 * 15.8]/221
n = 131.36/221
n = 0.594 mol