Answer: 1.99 x 10²² molecules H2
Explanation:First we will solve for the moles of H2 using Ideal gas law PV= nRT then derive for moles ( n ).
At STP, pressure is equal to 1 atm and Temperature is 273 K.
Convert volume in mL to L:
750 mL x 1 L / 1000 mL
= 0.75 mL
n = PV/ RT
= 1 atm ( 0.75 L ) / 0.0821 L.atm/ mole.K ( 273 K)
= 3.3x10-² moles H2
Convert moles of H2 to atoms using Avogadro's Number.
3.3x10-² moles H2/ 6.022x10²³ atoms H2 / 1 mole H2
= 1.99x10²² atoms H2
The factors that affect the rate of solution formation are capable of either increasing the rate of solution formation or decreasing it.
<h3>Factors that affect the rate of solution formation</h3>
The rate of solution formation from a chemical reaction depends on the following factors:
- Quantity of solute and solvent: The solute should be in less quantity and solvent should be more in quantity to dissolve the solute. This will enhance the formation of solution
- The size of the solute particles: When the solute particles are in smaller sizes, they react faster with the solvent to form solutions.
- The temperature of solvent: In increased temperature, the solute reacts faster with the solvent.
Therefore, the factors that affect the rate of solution formation are capable of either increasing the rate of solution formation or decreasing it.
Learn more about solutions here:
brainly.com/question/23946616
Answer:
P2= 45.50 atm
Explanation:
If the amount of gas in the tanks remains same we use the equation P1T1=P2T2
40 x 281.15 = P2 x 247.15
P2= 45.50 atm
Answer:
Here's what I get
Explanation:
I think this may be the equation you intended to write:
C₃H₅(OH)₃ + 3HCl ⟶ C₃H₅Cl₃ + 3H₂O
The mole ratios are the ratios of the coefficients in the balanced equation.
Here are some of the possible molar ratios.
- C₃H₅(OH)₃:HCl = 1:3
- C₃H₅(OH)₃:C₃H₅Cl₃ = 1:1
- C₃H₅(OH)₃:H₂O = 1:3
- HCl:C₃H₅Cl₃ = 3:1
- HCl:H₂O = 3:3
- C₃H₅Cl₃:H₂O = 1:3
Answer:
Rate = k . [B]² . [C]
Explanation:
The dependence of the reaction rate on the concentration of the reactants is given by the reaction order of each one, as shown in the rate equation.
![Rate=k.[A]^{x} .[B]^{y} .[C]^{z}](https://tex.z-dn.net/?f=Rate%3Dk.%5BA%5D%5E%7Bx%7D%20.%5BB%5D%5E%7By%7D%20.%5BC%5D%5E%7Bz%7D)
where,
k is the rate constant
x, y, z are the reaction orders.
- <em>The rate of reaction is not affected by changing the concentration of species A.</em> This means that the reaction order for A is x = 0 since when its concentration changes, the rate stays the same.
- <em>Leaving all other factors identical, doubling the concentration of species B increases the rate by a factor of 4.</em> This means that the reaction order for B is y = 2, so when the concentration is doubled, the new rate is 2² = 4 times the initial rate.
- The rate of the reaction is linearly dependent on the concentration of C. This means that the reaction order for C is z = 1, that is, a linear dependence.
All in all, the rate equation is:
Rate = k . [B]² . [C]
