1.679 × 10²³ g of PbO₂ is present in 4.23×10⁴⁴ particles of PbO₂.
<u>Explanation:</u>
First the number of particles is converted into moles by dividing it by the Avogadro's number and then moles multiplied by the molar mass, we will get the mass of PbO₂ in grams.
4.23×10⁴⁴/ 6.022×10²³ = 7.02×10²⁰ moles
Now we have to multiply this by the molar mass of PbO₂, that is 239.2 g/mol, we will get the mass in grams.
7.02×10²⁰ moles × 239.2 g/mol = 1.679 × 10²³ g of PbO₂
Answer:
No heat is released.
Explanation:
A substance absorbs heat when it melts.
The formula for the heat absorbed is
Data:
m = 10 g
\Delta_{fus) H=\text{334 J/g}
Calculations:
Answer:
Part A
Given that the graph is symmetrical and bell shaped, the average kinetic energy is given by the midline of graph, which corresponds to the common speed of the highest number of the population
Part B
The formula for the average kinetic energy, K.E. = (3/2)·(R/NA)·T
Therefore, the part of the graph that indicates the temperature of the sample is the average kinetic energy. K.E.
Part C
At a lower temperature, the heat is less evenly distributed and we have the distribution T2 higher than T1
Please see the attached graph created with MS Visio
Explanation:
The answer to “An iron nail with a mass of 12 g absorbs 15 J of heat. If the nail was initially at 28 °C, what is its final temperature?” is broken down into a number of easy to follow steps, and 27 words. Since the solution to 81P from 3 chapter was answered, more than 4841 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 81P from chapter: 3 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: nail, iron, heat, initially, final. This expansive textbook survival guide covers 19 chapters, and 2045 solutions.
Answer:
The value of the gas equilibrium constant Kp is 18.3
Explanation:
Step 1: Data given
Kp= Kc(RT)^Δn
Temperature = 298 K
Kc = 18.3
Step 2: The balanced equation
C₄(s) + 4 O₂(g) ⇌ 4 CO₂(g)
Step 3: Calculate Kp
Kp= Kc(RT)^Δn
⇒with Kp = the gas equilibrium constant = TO BE DETERMINED
⇒with Kc = the equilibrium constant = 18.3
⇒R = the gas constant = 0.08206 L* atm/mol*K
⇒T = the temperature = 298 K
⇒Δn = mol gas phase product – mol gas phase reactant = 4-4 =0
Kp = 18.3 * (0.08206*298)^0
Kp = 18.3 * 1
Kp = 18.3
The value of the gas equilibrium constant Kp is 18.3
