I hope this helps in some way. I forgot to mention that the question states they want to find THE NUMBER OF MOLES for H2O. Yherefore, you would want mol of H2O on top.
Answer:
<u></u>
Explanation:
<u>1. Balanced molecular equation</u>
![2HNO_3+Ba(OH)_2\rightarrow Ba(NO_3)_2+2H_2O](https://tex.z-dn.net/?f=2HNO_3%2BBa%28OH%29_2%5Crightarrow%20Ba%28NO_3%29_2%2B2H_2O)
<u>2. Mole ratio</u>
![\dfrac{2molHNO_3}{1molBa(OH)_2}](https://tex.z-dn.net/?f=%5Cdfrac%7B2molHNO_3%7D%7B1molBa%28OH%29_2%7D)
<u>3. Moles of HNO₃</u>
- Number of moles = Molarity × Volume in liters
- n = 0.600M × 0.0100 liter = 0.00600 mol HNO₃
<u>4. Moles Ba(OH)₂</u>
- n = 0.700M × 0.0310 liter = 0.0217 mol
<u>5. Limiting reactant</u>
Actual ratio:
![\dfrac{0.0600molHNO_3}{0.0217molBa(OH)_2}\approx0.28](https://tex.z-dn.net/?f=%5Cdfrac%7B0.0600molHNO_3%7D%7B0.0217molBa%28OH%29_2%7D%5Capprox0.28)
Since the ratio of the moles of HNO₃ available to the moles of Ba(OH)₂ available is less than the theoretical mole ratio, HNO₃ is the limiting reactant.
Thus, 0.006 moles of HNO₃ will react completely with 0.003 moles of Ba(OH)₂ and 0.0217 - 0.003 = 0.0187 moles will be left over.
<u>6. Final molarity of Ba(OH)₂</u>
- Molarity = number of moles / volume in liters
- Molarity = 0.0187 mol / (0.0100 + 0.0031) liter = 0.456M
The volume that would be occupied by 0.25 moles sample of H2 is calculated using ideal gas equation formula
that is PV =nRT
P(pressure)= 1.7 atm
V( volume)?
n(number of moles)= 0.250 moles
R(gas constant)=0.0821 l.atm/mol.K
T (temperature in kelvin)=35+273 = 308k
by making V the subject of the formula V=nRT/P
=(0.250 moles x 0.0821 L.atm/k.mol x 308 k)/( 1.70 atm) = 3.7 L of H2 gas
C. two billiard balls colliding and bouncing off each other
Explanation:
From the given options, the most similar scenario to the type of collision depicted in the kinetic molecular theory is the collision of the two billiard balls bouncing off each other.
Here are some of the postulates of the kinetic molecular theory:
- A gas is composed of a large number of identical molecules moving at different speeds.
- The space occupied by the gas molecules is negligible compared to the volume of the container.
- Molecules move independently of one another
- Molecules collides with one another and with the walls of the container elastically i.e without loss of kinetic energy.
- The temperature of the gas is a measure of its average kinetic energy.
Learn more;
Kinetic molecular theory brainly.com/question/12362857
#learnwithBrainly
<h3>
Answer:</h3>
18.02 g/mol
<h3>
General Formulas and Concepts:
</h3>
<u>Math</u>
<u>Pre-Algebra</u>
Order of Operations: BPEMDAS
- Brackets
- Parenthesis
- Exponents
- Multiplication
- Division
- Addition
- Subtraction
<u>Chemistry</u>
<u>Atomic Structure</u>
<h3>Explanation:
</h3>
<u>Step 1: Define</u>
Water H₂O
<u>Step 2: Find Formulas Mass</u>
<em>Formula mass is molar mass.</em>
Molar Mass of H - 1.01 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol