Consider the following reaction: Calculate the amount of heat transferred when 3.53 g of Mg(s) reacts at constant pressure. Express your answer in kilojoules to three significant figures. 2Mg(s) + Oz(g) → 2MgO(s), AH=-1204 kJ AH - kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining • Part C How many grams of MgO are produced during an enthalpy change of -235 kJ ? Express your answer in grams to three significant figures. ? Submit Request Answer • Part D How many kilojoules of heat are absorbed when 40.4 g of MgO(s) is decomposed into Mg(s) and O2(g) at constant Express your answer in kilojoules to three significant figures. ΔΗ. kJ Submit Request Answer

Consider the following reaction: Calculate the amount of heat transferred when 3.53 g of Mg(s) reacts at constant pressure. Express your answer in kilojoules to three significant figures. 2Mg(s) + Oz(g) → 2MgO(s), AH=-1204 kJ AH - kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining • Part C How many grams of MgO are produced during an enthalpy change of -235 kJ ? Express your answer in grams to three significant figures. ? Submit Request Answer • Part D How many kilojoules of heat are absorbed when 40.4 g of MgO(s) is decomposed into Mg(s) and O2(g) at constant Express your answer in kilojoules to three significant figures. ΔΗ. kJ Submit Request Answer

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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A chemist measures the energy change AH during the following reaction: CH₂(g) +20₂(g) → CO₂(g) + 2H₂O(l) Use the information to answer the following questions. This reaction is... Suppose 37.8 g of CH₁ react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. AH = -882. kJ endothermic. O exothermic. OYes, absorbed. O Yes, released. O No. kJ x10 Start over Ś
A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q = specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the sblution increases to 30.0 °C At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, qp; that is, Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water (4.18 J/(g. °C)J, that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. ΔΗp Express the…
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
Suppose that the molar enthalpy of a reaction is -69.06 kJ/mol and 1.134 moles are reacted. How many kilojoules of heat are released by the reaction? Report your answer to three decimal places (ignore significant figures).
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Consider the following reaction. N2 + 3 H2 -> 2 NH3 ΔH = -92 kJ/mol If 35 g of NH3 are produced, then what amount of heat energy is released?
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The answer is 44.8 kJ/mol. Show the solution how to get 44.8 kJ/mol.
Which chemical reaction below yields the heat of formation of liquid ammonia (NH3)? 3H(g) + N(g) →→→ NH3(e) H₂ (g) + N2₂ (g)→→ NH3(e) 3/2 H₂ (g) + 1/2 N₂ (g)→ NH3 (e) 3H₂(g) + N₂ (g)→ 2NH3(e) 3/2 H₂(g) + N(g)→ NH3(e)
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