<span> A homogeneous mixture is composed of a single visible phase while a heterogeneous mixture has two or more</span>
These problems are a bit interesting. :)
First let's write the molecular formula for ammonium carbonate.
NH4CO3 (Note! The 4 and 3 are subscripts, and not coefficients)
17.6 gNH4CO3
Now to convert to mol of one of our substances we take the percent composition of that particular part of the molecule and multiply it by our starting mass. This is what it looks like using dimensional analyse.
17.6 gNH4CO3 * (Molar Mass of NH4 / Molar Mass of NH4CO3)
Grab a periodic table (or look one up) and find the molar masses for these molecules! Well. In this case I'll do it for you. (Note: I round the molar masses off to two decimal places)
NH4 = 14.01 + 4*1.01 = 18.05 g/mol
NH4CO3 = 14.01 + 4*1.01 + 12.01 + 3*16.00 = 78.06 g/mol
17.6 gNH4CO3 * (18.05 molNH4 / 78.06 molNH4CO3)
= 4.07 gNH4
Now just take the molar mass we found to convert that amount into moles!
4.07 gNH4 * (1 molNH4 / 18.05 gNH4) = 0.225 molNH4
Answer:
Yes
Explanation:
because some foods have carbohydrates but are healthy
Answer:
Molar mass of solute: 300g/mol
Explanation:
<em>Vapor pressure of pure benzene: 0.930 atm</em>
<em>Assuming you dissolve 10.0 g of the non-volatile solute in 78.11g of benzene and vapour pressure of solution was found to be 0.900atm</em>
<em />
It is possible to answer this question based on Raoult's law that states vapor pressure of an ideal solution is equal to mole fraction of the solvent multiplied to pressure of pure solvent:
Moles in 78.11g of benzene are:
78.11g benzene × (1mol / 78.11g) = <em>1 mol benzene</em>
Now, mole fraction replacing in Raoult's law is:
0.900atm / 0.930atm = <em>0.9677 = moles solvent / total moles</em>.
As mole of solvent is 1:
0.9677× total moles = 1 mole benzene.
Total moles:
1.033 total moles. Moles of solute are:
1.033 moles - 1.000 moles = <em>0.0333 moles</em>.
As molar mass is the mass of a substance in 1 mole. Molar mass of the solute is:
10.0g / 0.033moles = <em>300g/mol</em>
The volume of a 14.00g of nitrogen at 5.64atm and 315K is 4.59L.
<h3>How to calculate volume?</h3>
The volume of an ideal gas can be calculated using the following ideal gas equation formula;
PV = nRT
Where;
- P = pressure (atm)
- V = volume (L)
- n = number of moles
- R = gas law constant
- T = temperature
An ideal gas is a hypothetical gas, whose molecules exhibit no interaction, and undergo elastic collision with each other and with the walls of the container.
The number of moles in 14g of nitrogen can be calculated as follows:
moles = 14g ÷ 14g/mol = 1mol
5.64 × V = 1 × 0.0821 × 315
5.64V = 25.86
V = 25.86 ÷ 5.64
V = 4.59L
Therefore, 4.59L is the volume of the gas
Learn more about volume at: brainly.com/question/12357202
#SPJ1
