Ferrous sulfate (molar mass 152 g/mol) is a medicine used to treat anaemia. On heating it decomposes to produce ferric oxide, sulfur dioxide and sulfur trioxide. 2FeSO4 (s) Fe2O3 (s) + SO₂ (g) + SO3 (9) Which ONE represents the work done during the decomposition of 30.4 g of ferrous sulfate at 1 atm (101325 Pa) and 298 K? -248 J -496 J 496 J 248 J OJ →

Ferrous sulfate (molar mass 152 g/mol) is a medicine used to treat anaemia. On heating it decomposes to produce ferric oxide, sulfur dioxide and sulfur trioxide. 2FeSO4 (s) Fe2O3 (s) + SO₂ (g) + SO3 (9) Which ONE represents the work done during the decomposition of 30.4 g of ferrous sulfate at 1 atm (101325 Pa) and 298 K? -248 J -496 J 496 J 248 J OJ →

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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ulate het reaction enthalpy O O D Dwayne V Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) - CH,OH(1) + H,O(1) AH =-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH,OCH,(g) + H,0(1) AH - 8. kJ olb Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. Explanation Check O 2021 McGraw Hill LLC. All Rights Reserved. Terms of UseI Privacy Center Accessibility 4:25 AM ENG 12/14/2021 35°F Clear O Type here to search
When 1.16E-1 g of Zn(s) combines with 5.21E1 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 2.34E1 °C to 2.46E1 °C:Zn(s) + 2HCl(aq) → ZnCl(aq) + H(g) Calculate the enthalpy change of the reaction ΔH in J/mol. (Assume the volume of the solution doesn't change, density of the solution is 1.00 g/mL and the specific heat capacity of solution is 4.184 J/g°C.)
When chemical A and chemical B are mixed together, and endothermic reaction below occurs:4A(aq) + 3B(s) --> 2C(aq)To find the enthalpy of this reaction, a scientist pours 155 mL of a 0.33 M solution A into abeaker and measures the temperature to be 20.1 ̊C. To this same beaker the scientist thenadds 3.75 g of substance B with stirring (molar mass of B is 33 g/mol), and finds thetemperature to now be 16.3 ̊C. Calculate the molar enthalpy of this reaction for every mole ofC produced.
Butane, C4H10, is widely used as a fuel for disposable lighters When one mole of butane is burned in oxygen, carbon dioxide and steam are formed and 2654.3382 kJ of heat are evolved.. C4H10 (9) + O₂(g) → 4CO₂(g) +5H₂O(1) The standard enthalpies of formation of CO₂ and H₂O are: CO2(g)=-394.87 kJ/mol H₂O(1)=-285.59 kJ/mol Calculate the standard heat of formation of butane. (Round answer to the second decimal place)
Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer
To study the possible amount of energy generated by a person, the person can be roughly viewed as a constant pressure calorimeter using table sugar (sucrose, C12H22O11) as the energy generator. The reaction of table sugar in a calorimeter is given by: C12H22O11(s) + 12O2(g) ----------> 12CO2(g) + 11H2O(g) a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. Calculate the enthalpy of combustion per mole of sugar utilization. c. Does the result of your calculation make sense?
A gas expands from 287 mL to 959 mL at a constant temperature. Calculate the work done (in joules) by the gas if it expands (a) against a vacuum. W = J (b) against a constant pressure of 4.00 atm. W = J
Decaborane-14 (B₁H₁4) is a white, highly reactive solid that will burst into flames when exposed to oxygen. The reaction is B₁H₁(g) + 110₂(g) SB₂0,(s) + 7H₂0 (1) Calculate the kilojoules of heat released per gram of the compound reacted with oxygen. The standard enthalpy of formations of B, H₁ (s), B₂O, (s), 0, (g) , and H₂O (/) are 82.8 kJ mol -1273.5 kJ kJ 0 mol' mol' 4 kJ 1- released 8 B. H.. 10 14 and-285.8 2 kJ mol respectively. Round your answer to 1 decimal place.
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When methanol, CH3OH,CH3OH, is burned in the presence of oxygen gas, O2,O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJCH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJ How much methanol, in grams, must be burned to produce 639 kJ639 kJ of heat?
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