## Extensive Property**Given:**- 3.93 g of methanol ($CH_3OH$)- 6.36 g of oxygen gas ($O_2$)These reactants are allowed to react. ### d.1 Determine the mass of each reactant and product after complete reaction. Use the reaction table to find the limiting reactant and mass of products.#### Reaction:\[2CH_3OH + 3O_2 \rightarrow 2CO_2 + 4H_2O\]\[ \text{Mass of methanol used: } 3.93 \text{ g} \]\[ \text{Mass of oxygen used: } 6.36 \text{ g} \]### d.2 The heat released during this combustion.### d.3 If the heat above is absorbed by a Styrofoam calorimeter containing 300 g of water at 25°C, what will be the final temperature of the water? Assume the calorimeter heat capacity is 15.0 J/°C.### Explanation Diagrams1. **Chemical Equation:** The balanced chemical equation for the combustion of methanol is written: \[2CH_3OH + 3O_2 \rightarrow 2CO_2 + 4H_2O\]2. **Mass Conversion Diagram:** - Given masses and molar masses are used to convert grams to moles for both methanol and oxygen. - Determine the limiting reactant based on molar ratios. - Calculate the mass of CO2 and H2O produced upon complete reaction.3. **Heat Calculation:** - Using given/molar enthalpies and mass of reactants, the heat released (\[ \Delta H \]) is determined. - This heat release can be applied through specific heat capacity equation to determine rise in temperature of the water.These diagrams/steps ensure a step-by-step approach to solving the reaction and heat absorption problem.

Amount of methanol = 3.93 g.Amount of oxygen = 6.36 g.

(nolond briod) valadina in (d) [Extensive Property] Given 3.93 g of methanol and 6.36g of oxygen gas are allowed to 2CH3OH+302 → 200₂ + 4H₂O react, determine d.1 d.2 The mass of each reactant and product after complete reaction. Use the reaction table to find limiting reactant and mass of products. CHOC The heat released during this combustion. 6.36g. Imel 16 g/mol d.3 If the heat above is absorbed by a Styrofoam calorimeter containing 300.0g of water at 25°C, what will be the final temperature of the water? Assume the calorimeter heat capacity is 15.0 J/°C.

(nolond briod) valadina in (d) [Extensive Property] Given 3.93 g of methanol and 6.36g of oxygen gas are allowed to 2CH3OH+302 → 200₂ + 4H₂O react, determine d.1 d.2 The mass of each reactant and product after complete reaction. Use the reaction table to find limiting reactant and mass of products. CHOC The heat released during this combustion. 6.36g. Imel 16 g/mol d.3 If the heat above is absorbed by a Styrofoam calorimeter containing 300.0g of water at 25°C, what will be the final temperature of the water? Assume the calorimeter heat capacity is 15.0 J/°C.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

## Extensive Property

**Given:**
- 3.93 g of methanol ($CH_3OH$)
- 6.36 g of oxygen gas ($O_2$)

These reactants are allowed to react.

### d.1 Determine the mass of each reactant and product after complete reaction. Use the reaction table to find the limiting reactant and mass of products.

#### Reaction:
\[2CH_3OH + 3O_2 \rightarrow 2CO_2 + 4H_2O\]

\[ \text{Mass of methanol used: } 3.93 \text{ g} \]
\[ \text{Mass of oxygen used: } 6.36 \text{ g} \]

### d.2 The heat released during this combustion.

### d.3 If the heat above is absorbed by a Styrofoam calorimeter containing 300 g of water at 25°C, what will be the final temperature of the water? Assume the calorimeter heat capacity is 15.0 J/°C.

### Explanation Diagrams
1. **Chemical Equation:**
The balanced chemical equation for the combustion of methanol is written:
\[2CH_3OH + 3O_2 \rightarrow 2CO_2 + 4H_2O\]

2. **Mass Conversion Diagram:**
- Given masses and molar masses are used to convert grams to moles for both methanol and oxygen.
- Determine the limiting reactant based on molar ratios.
- Calculate the mass of CO2 and H2O produced upon complete reaction.

3. **Heat Calculation:**
- Using given/molar enthalpies and mass of reactants, the heat released (\[ \Delta H \]) is determined.
- This heat release can be applied through specific heat capacity equation to determine rise in temperature of the water.

These diagrams/steps ensure a step-by-step approach to solving the reaction and heat absorption problem.

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