1 Consider the following reaction H14x a Is the reaction end

1. Consider the following reaction: H=-1.4x a. Is the reaction endothermic or exothermic? b. If this reaction was run in a calorimeter would the temperature of the calorimeter contents increase or decrease? 75.0 g of C,H,OH were reacted with excess 0x(g) according to the above reaction. Calculate the kJ of heat transferred. c. 2. In each of the following reactions, identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent. a. 2Ca(s) + O2(g) 2CaO(s) b. 2Cs(s) +Cl2(g) 2CsCI(s) c. Zn + H2SO4 ZnSO4 + H2 d. 2Nal + Br2 2NaBr +12

Solution

Hi as per Chegg guidelines we can answer only one full question, but i am answering two questions for you,please post remaining questions seperately.

1 a) exothermic reaction. Since the enthalpy change H has neagtive sign, by definition it is exothermic.

1 b) temperature of the calorimeter increases, since exothermic reactions releases heat energy.

1 c) from given balanced chemical reaction equation 1mol C₂H₅OH gives 1.4 x 10³ kJ energy. We have to calculate how many moles are present in 75g of C₂H₅OH.

moles C₂H₅OH = mass of C₂H₅OH / molar mass of C₂H₅OH = 75g / 46.07 g/mol = 1.62795745605 mol

multiply moles C2H5OH with  1.4 x 10³ kJ = 1.62795745605 x 1.4 x 10³ kJ = 2.3 x 10³ kJ

heat transferred = 2.3 x 10³ kJ

2a) Ca(s) oxidized and reducing agent; O₂(g) is reduced and oxidizing agent.

2b) Cs(s) oxidized and reducing agent; Cl₂(g) is reduced and oxidizing agent.

2c) Zn oxidized and reducing agent; H⁺ is reduced and oxidizing agent.

2d) I^- oxidized and reducing agent; Br₂(g) is reduced and oxidizing agent.

oxidized = loss of electrons; reduced = gain of electrons; oxidizing agent = removes electrons from other species; reducing agent = gives electrons to other species.

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