(a) Write the balanced chemical equation that represents the standard heat of formation of Cu,0(s) at 298 K. Be sure to specify states. Write fractions with a slash, such as 1/2 for one half. If a box is not needed leave it blank. + (b) The standard enthalpy change for the following reaction is -1.20x10 kJ at 298 K. 2 Be(s) + O2(g)-2 BeO(s) What is the standard heat of formation of BeO(s)? kJ/mol Check & Submit Answer Show Approach

(a) Write the balanced chemical equation that represents the standard heat of formation of Cu,0(s) at 298 K. Be sure to specify states. Write fractions with a slash, such as 1/2 for one half. If a box is not needed leave it blank. + (b) The standard enthalpy change for the following reaction is -1.20x10 kJ at 298 K. 2 Be(s) + O2(g)-2 BeO(s) What is the standard heat of formation of BeO(s)? kJ/mol Check & Submit Answer Show Approach

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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Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
2. (a) 36 mL of 1.0M hydrochloric acid is react with a solution of sodium hydroxide of the concentration 1.6M and volume 15 mL in a coffee cup calorimeter. It is noted that the temperature of both solutions before the reaction is 27.5 °C. After the reaction, the temperature of the solution raise to 35.0 °C. Calculate heat of neutralization for the reaction.(cw = 4.18 Jgl°C', Density of solution: 1gmL').
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ ((b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 880.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
When 2.232 g of AX (s) dissolves in 147.5 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 34.8 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: · The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL · The liquid's final volume is not changed by adding the solid · The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
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You wish to know the enthalpy change for the formation of liquid PCI, from the elements. P.()+6 Cl₂(g) →4 PC (6) A, H-7 The enthalpy change for the formation of PCs from the elements can be determined experimentally, as can the enthalpy change for the reaction of PCs (f) with more chlorine to give PCI, (s): P.()+10 Cl₂(g) 4 PCI, () A,H-1774.0 kJ/mol-rxn PCI, ()+ Cl₂(g) → PCI, (s) - A,H-123.8 kJ/mol-rxn Use these data to calculate the enthalpy change for the formation of 2.20 mol of PCs (4) from phosphorus and chlorine. Enthalpy change - k3
Calculate the standard enthalpy of formation for C3H6O (l) from its combustion using the following data: Enthalpy of this combustion is -1793 kJ ( you must write a balanced reaction first).
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When 0.215 g of sodium metal is added to an excess of hydrochloric acid, 2230 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HC1(aq) 2 NaCI(aq) + H, (g) Enthalpy of reaction: kJ
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
You wish to know the enthalpy change for the formation of liquid PC13 from the elements. P4(s) + 6 Cl2 (g) → 4 PC13 (€) A, H' =? The enthalpy change for the formation of PCI5 from the elements can be determined experimentally, as can the enthalpy change for the reaction of PCI3 (() with more chlorine to give PCI5 (s): P4(s) + 10 Cl2 (g) → 4 PCI5 (s) A,H = -1774.0 kJ/mol – rxn PCI3 (e) + Cl2 (g) → PC15 (s) A,H° = -123.8 kJ/mol – rxn Use these data to calculate the enthalpy change for the formation of 3.60 mol of PCI3 (€) from phosphorus and chlorine. Enthalpy change = | kJ