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Zielflug [23.3K]
3 years ago
8

Drag the correct symbol to the equation. Not all symbols will be used.

Chemistry
1 answer:
nikklg [1K]3 years ago
6 0

Answer:

  • ¹⁰³₄₀ Zr

Explanation:

The nuclear equation from which you have to identify the missing element is:

  • ²³⁹₉₄ Pu + ¹₀n → ___ + ¹³⁴₅₄Xe + 3 ¹₀n

The superscripts to the left of each chemical symbol are the mass number of the atoms (number of protons plus neutrons) and the subscripts to the left of the chemical symbols are the atomic numbers of the atoms (number of protons).

Thus, such equation must be read as "an atom of plutonium-239 is bombarded with a neutron and produces one atom of an unkwon element, one atom of xenon-134, and 3 neutrons".

To find the identity of the missing element you must do two balances: mass number and atomic number.

Mass number:

  • 239 + 1 = A + 134 + 3×1
  • A = 240 - 134 - 3 = 103

Hence, the mass number of the missing element is 103.

Atomic number:

  • 94 + 0 = Z + 54 + 3×0
  • Z = 94 - 54 = 40

Hence, the atomic number of the missing element is 40.

In a periodic table you can find that the element with atomic number 40 is zirconium, Zr.

Thus, the identity of the missing isotope is zirconium-103, ¹⁰³₄₀Zr.

And the complete equation is:

  • ²³⁹₉₄ Pu + ¹₀n →  ¹⁰³₄₀ Zr + ¹³⁴₅₄Xe + 3 ¹₀n
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Water has a heat of fusion of about 300J/gram and a heat capacity for liquid water of a about 4J/gC. How much heat is needed to
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Answer:

The total heat required is 3.4 kJ

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

There is a direct proportional relationship between heat and temperature. So, the amount of heat a body receives or transmits is determined by:

Q = c * m * ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case you know;

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Replacing:

Q= 4\frac{J}{g*C} *10 g * 10 C

Solving:

<em>Q1= 400 J</em>

On the other hand, you must determine the heat required to convert 0 ∘ C of ice to 0 ∘ C of liquid water by:

Q2=m*heat of fusion

Q2=10 g* 300 \frac{J}{g}

<em>Q2= 3,000 J</em>

The total heat required is:

Q= Q1 + Q2= 400 J + 3,000 J

Q= 3,400 J= 3.4 kJ (1 kJ= 1,000 J)

<u><em>The total heat required is 3.4 kJ</em></u>

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H2(g) + Cl2 (g) → 2HCl (g)

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