Decay constant of the process 1×10^(-12) day^(-1).
<h3>What is decay constant?</h3>
A radioactive nuclide's probability of decay per unit time is known as its decay constant, which is expressed in units of s1 or a1. As a result, as shown by the equation dP/P dt =, the number of parent nuclides P declines with time t. Nuclear forces are about 1,000,000 times more powerful than electrical and molecular forces in their ability to bind protons and neutrons. The strength of the bonds holding the radioactive element are likewise indifferent to the decay probabilities and's, in addition to being unaffected by temperature and pressure. The decay constant is related to the nuclide's T 1/2 half-life by T 1/2 = ln 2/.
To know more about decay constant:
brainly.com/question/16623902
#SPJ4
Answer:
International System of Units (SI)
Explanation:
I hope it helps :)
When energy transforms into mass, the amount of energy does not remain the same. When mass transforms into energy, the amount of energy also does not remain the same. However, the amount of matter and energy remains the same. ... You would weigh much less on the Moon because it is only about one-sixth the mass of Earth. So the answer is D
Answer:
The answer to your question is C = 0.037 cal/g°C
Explanation:
Data
mass of the wire = m = 237 g
temperature 1 = T1 = 25°C
temperature 2 = T2 = 107°C
Heat = Q = 722 cal
Specific heat = C
Process
1.- Write the formula to find the specific heat
Q = mC(T2 - T1)
-Solve for C
C = Q / m(T2 - T1)
2.- Substitution
C = 722 / 237(107 - 25)
3.- Simplification
C = 722 / 237(82)
C = 722 / 19434
4.- Result
C = 0.037 cal/g°C
Answer:
The molarity of this solution is 0.156 M
Explanation:
Step 1: Data given
Mass of Ba(OH)2 = 1.90 grams
Molar mass Ba(OH)2 = 171.34 g/mol
Volume of the solution = 71.1 mL = 0.0711 L
Step 2: Calculate moles Ba(OH)2
Moles Ba(OH)2 = mass Ba(OH)2 / molar mass Ba(OH)2
Moles Ba(OH)2 = 1.90 grams / 171.34 g/mol
Moles Ba(OH)2 = 0.0111 moles
Step 3: Calculate molarity
Molarity solutin = moles Ba(OH)2 / volume solution
Molarity solution = 0.0111 moles / 0.0711 L
Molarity solution = 0.156 M
The molarity of this solution is 0.156 M
