Answer: 1.52 atm
Explanation:
Given that:
Volume of gas V = 10.0L
Temperature T = 35.0°C
Convert Celsius to Kelvin
(35.0°C + 273 = 308K)
Pressure P = ?
Number of moles = 0.6 moles
Molar gas constant R is a constant with a value of 0.0821 atm L K-1 mol-1
Then, apply ideal gas equation
pV = nRT
p x 10.0L = 0.6 moles x (0.0821 atm L K-1 mol-1 x 308K)
p x 10.0L = 15.17 atm L
p = 15.17 atm L / 10.0L
p = 1.517 atm (round to the nearest hundredth as 1.52 atm)
Thus, the pressure of the gas is 1.52 atm
I can't see the picture, it's too small and grainy...
>.<
I would go with false but idk
Answer:
0.023
Explanation:
The Arrhenius' equation states that:
Where k is the velocity constant of the reaction, A is the constant of the collisions, Ea is the activation energy (the energy necessary to the molecules have so the reaction will happen), R is the gas constant (8.314 J/molK) and T is the temperature.
This equation is derivated of:
k = pZf
Where
p=fraction of collisions that occur with reactant molecules properly oriented
f=fraction of collisions having energy greater than the activation energy
Z=frequency of collisions
Thus, p*Z = A, and
f =
So, if the energy of the molecules is 12.5 kJ/mol = 12500 J/mol, thus the fraction will be:
f =
f = 0.023
Answer:
Explanation:
1. The reaction will proceed backward, shifting the equilibrium position to the left.
2. The reaction will proceed forward, shifting the equilibrium position to the right.
3. Either add more of the products ( H2O or Cl2) or remove the reactant (HCl or O2)