Write balanced equations for (a) 238922U + 1n -> 224194Pu. (b) 147N + 1a -> 1p + 178O. (c) 5626Fe + 1a -> 1b + 6029Cu.

Verified step by step guidance

Step 1: Identify the type of nuclear reaction for each equation. For example, determine if it is a fission, fusion, or decay process.

Step 2: For each equation, ensure that the sum of atomic numbers (subscripts) and mass numbers (superscripts) are equal on both sides of the equation. This is based on the law of conservation of mass and charge.

Step 3: For equation (a), balance the equation by adding the appropriate particles (such as neutrons or protons) to ensure both sides have equal atomic and mass numbers.

Step 4: For equation (b), balance the equation by identifying the missing particle (1a) and ensuring the atomic and mass numbers are balanced on both sides.

Step 5: For equation (c), determine the identity of the missing particle (1b) by balancing the atomic and mass numbers, ensuring the equation is balanced.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Nuclear Reactions

Nuclear reactions involve changes in an atom's nucleus and can result in the transformation of one element into another. They typically include the emission or absorption of particles such as neutrons (n), alpha particles (α), and beta particles (β). Understanding the types of nuclear reactions is essential for balancing equations, as it helps identify the reactants and products involved.

Balancing Nuclear Equations

Balancing nuclear equations requires ensuring that both the mass number and atomic number are conserved during the reaction. This means that the sum of the mass numbers and the sum of the atomic numbers on the reactant side must equal those on the product side. Mastery of this concept is crucial for accurately writing and interpreting nuclear equations.

Isotopes and Atomic Notation

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers. Atomic notation, which includes the element symbol, mass number, and atomic number, is used to represent isotopes. Familiarity with isotopes and their notation is vital for correctly identifying and writing nuclear reactions.

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Textbook Question

Complete and balance the following nuclear equations by supplying the missing particle: (a) 147N + 42He¡? + 11H

Textbook Question

Complete and balance the following nuclear equations by supplying the missing particle: (d) 5826Fe + 2 10n¡6027Co + ?

Textbook Question

Complete and balance the following nuclear equations by supplying the missing particle: (e) 23592U + 10n¡13554Xe + 2 10n + ?

Textbook Question

Each statement that follows refers to a comparison between two radioisotopes, A and X. Indicate whether each of the following statements is true or false. (a) If the half-life for A is shorter than the half-life for X, A has a larger decay rate constant.

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