Maganiussam hydroclroid has is produced
I believe this is the answer
To solve this item, we need write first all the necessary data to solve the problem. Governing principle of this problem is basically exponential decay of a certain substance.
Given:
Let t represents time
N represents mass of substance
Initially,
at t(0), N(0) = 190mg radioactive substance
at t(17), N(17) = 95mg radioactive substance
Required: N(21)
Solution:
We write first the formula for exponential decay, that is
N(t) = N(0)*e^(-k*t) ; k = exponential decay constant
We need first to determine the k, substituting the given we have
95 = 190*e^(-k*17)
Dividing by 190, we get
0.5 = e^(-k*17)
To eliminate the exponential e, we take the natural logs of both sides
ln(0.5) = ln(e^(-k*17))
-0.693 = -k*17
Solving for k,
k = 0.04077
To solve for N(21), we need to substitute k to the original equation
N(21) = N(0)e^(-k*21)
N(21) = 190*e^(-0.04077*21)
N(21) = 80.7 mg
<em>ANSWER: 80.7 mg radioactive substance left after 21 hours </em>
Answer:
None
Explanation:
None of these equations are balanced. To determine if an equation is balanced, count the number of each element on each side. If the product side (right) equals the reactant side (left), then an equation is balanced.
To count atoms, multiply its subscript (the small number if it has one) with the coefficient (the big number if it has one).
C + S => CS₂
C 1 C 1
S 1 S 2
The "S" sulphur atoms are not balanced.
25O₃ => 25O₂ + O₂
O 75 O 52
The "O" oxygen atoms are not balanced.
2NH₃ => N₂+ 2H₂
N 2 N 2
H 6 H 4
The "H" hydrogen atoms are not balanced.
2C + O₂ => CO₂
C 2 C 1
O 2 O 2
The "C" carbon atoms are not balanced.
Balancing equations
Write coefficients until both sides have the same number of atoms. Each time you make a change, recount the number of atoms. Here are the balanced chemical equations: (I wrote in <u>bold and underline</u>)
C + <u>2</u>S => CS₂
<u>2</u>O₃ => <u>2</u>O₂ + O₂
2NH₃ => N₂ + <u>3</u>H₂
2C + <u>2</u>O₂ => <u>2</u>CO₂
Answer: The half-reaction correctly shows the oxidation of iron
Explanation:
Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.
Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.
The oxidation of iron is represented as:
Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.
The reduction of iron is represented as: