Nickel metal reacts with cadmium(II) nitrate reacts to produce cadmium metal and nickel(II) nitrate. Write the reaction equation on your scratch paper before answering this question. For this reaction Group of answer choices Ni is the reducing agent and it gains electrons. Cd2+ is the reducing agent and it loses electrons. Cd2+ is the oxidizing agent and it loses electrons. Cd2+ is the oxidizing agent and it gains electrons. Ni is the oxidizing agent and it loses electrons.

Imagine you were working as a laboratory technician and your principal investigator asked you to develop Benedict’s test into a quantitative measure of the concentration of reducing sugar in a solution. To do this, you would first need to decide what to measure and then establish the relationship between your measurements and different concentrations of reducing sugars. Explain generally what you would decide to measure and how you would go about determining the relationship of your measurements to the concentration of reducing sugar.

Determine which two of the following reactions are redox reactions. If the reaction is a redox reaction, indicate which element is being oxidized. Briefly explain your answers. Mg + Cl2 ⟶ MgCl2  MgO + 2HCl ⟶ MgCl2 + H2O  2CuCl2 + 4KBr ⟶ 2CuBr + 4KCl + Br2

Write balanced chemical equations for the following chemical reactions. A pure copper wire placed in an aqueous solution of silver nitrate produces a blue solution of copper (II) nitrate and powdered silver metal

Write the equation for the dissolving of iron(II) hydroxide in water. Be sure to specify the state of each reactant and product. +

Select the Single Replacement Reactions that WILL occur O NaCl + H2 -> HCI + Na O AgNO3 + Ca -> Ca(NO3)2 + Ag O Fe + MgSO4 -> FeSO4 + Mg O ZnCl2 + Cu -> CuCl2 + Zn

How would you classify the following chemical reaction? 2C8H18 (1) + 2502(g) → 16CO2(g) + 18H2O(1) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Acid-base neutralization Combustion C Oxidation-reduction Both B and C

Here is some information to help. In this experiment, magnesium metal is heated until it reacts with oxygen in the air according to the following balanced equation: 2Mg(s)+ O2(g) → 2MgO(s)                                                                  (silver metal)                  (white-gray ash) As the magnesium burns in air, it may also combine with nitrogen in air. To remove any nitride product, water is added, and the product is reheated. Any nitride product is converted to magnesium oxide and ammonia. 3Mg(s)+ N2(g) → Mg3N2(s) Mg3N2(s)+3H2O(l)→3MgO(s)+2NH3(aq) A weighed amount of the magnesium metal is used, and the mass of the oxide product formed is determined at the end of the experiment. The mass of oxygen that combines with the magnesium is obtained from the difference between the mass of the oxide product and the original mass of magnesium. mass of oxide product-mass of magnesium=mass of oxygen in oxide product The empirical formula of the oxide…

Consider the following redox reaction: 3Ag+ (aq) + Al(s) → 3Ag (s) + A1³+ (aq) If this reaction starts with 2.50 g of Al and the enough amount of Ag+, how much of electric charge could be generated? 4.28 x 104 C 8.94 × 10³ C 2.68 × 104 C 6.25 × 10³ C O 1.67 x 104 C

Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as chemical formulas. Omit states-of-matter. a. CO(g) + H₂O(g) → CO₂ (g) + H₂ (9) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced b. 3AgNO3(aq) + Sc(s) → Sc(NO3)3(aq) + 3Ag(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Submit Answer Try Another Version 1 item attempt remaining