unlv.instructure.com 7. Determine the change in enthalpy (AH) for the reaction:[1.5] CH3COCH3(1) +202(g) --> CH3COOH(I) + CO2(g) + H2O(g) Using the given information: CH3COCH3(1) +4 O2(g) --> 3 CO2(g) + 3 H20(I) AH = -1787.0 kJ H20(1) --> H2O(g) AH = -44.1 kJ CH3COOH(I) + 2 02(g) --> 2 CO2(g) + 2H2O(1) AH = -835.0 kJ 8.50.0 mL of 1.00 M HCI is mixed with 50.0 mL of 0.95 M KOH in a calorimeter with a caloriem constant (Kcall) of 17.3 J/°C. A change in temperature was observed from 26.0 °C to 32.6 °C. Wh

unlv.instructure.com 7. Determine the change in enthalpy (AH) for the reaction:[1.5] CH3COCH3(1) +202(g) --> CH3COOH(I) + CO2(g) + H2O(g) Using the given information: CH3COCH3(1) +4 O2(g) --> 3 CO2(g) + 3 H20(I) AH = -1787.0 kJ H20(1) --> H2O(g) AH = -44.1 kJ CH3COOH(I) + 2 02(g) --> 2 CO2(g) + 2H2O(1) AH = -835.0 kJ 8.50.0 mL of 1.00 M HCI is mixed with 50.0 mL of 0.95 M KOH in a calorimeter with a caloriem constant (Kcall) of 17.3 J/°C. A change in temperature was observed from 26.0 °C to 32.6 °C. Wh

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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PCIS(s) can be prepared by the reaction PCl3(0) + Cl2(g) PCls(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCIs(s) by the above reaction, given the following data. Pals) + 6 Cl2(g) -4 PCI3(1) AH° = -1280 kJ per mole of P4(s) Pa(s) + 10 Cl2(g) -4 PCI5(s) AH = -1774 kJ per mole of P4(s) -124 O-258 O+124 O+59.3 O-59.3
Calculate the enthalpy change for the following reaction, _C₂H4 (9) + using the following standard heats of formation: AH(C₂H4) = +52.5 kJ/mol; AH(CF4) =-933.0 kJ/mol; AH (HF) =-271.6 kJ/mol _F₂(g) → _CF4(g) + _HF(g)
4. Hess's Law Calculate AH for the reaction: 2 C(s) + H2(g) → C:H2(g), given the following chemical equations and their respective enthalpy changes: C2H2(g)+02(g)→2CO2(g)+H20(1) AH, = -1299.6 kJ (1) %3D C(s)+02(g)→CO2(g) AH, = -393.5 kJ (2) H2(g)+502(g)→H20(1) AH3 = -285.8 kJ (3)
Consider the following reaction: CH4 (9) + 20, (g) → CO2(g) + 2H,0(1) AH=-891 kJ a. Calculate the enthalpy change if 2.59 g methane is burned in excess oxygen. Enthalpy change = kJ b. Calculate the enthalpy change if 3.04 × 10° L methane gas at 737 torr and 25°C is burned in excess oxygen. Enthalpy change = kJ
For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of C, H₁g (g) consumed, under standard conditions. 25 Cg H18 (8) + O₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = $ V T B MacBook Air Y H & 7 8 AH-5108.7 kJ/mol 18 N M K 1 38 kJ/mol
Determine the enthalpy for the production of 5.0 g of H2 in the following target equation, making use of the known equations given below. CH4 (g) + NH3 (g) → HCN(g) + 3H2 (g) Using the following given equations: N2 (g)+3H2 (g) → 2NH3 (g) ΔH=− 91.8kJ C(s)+2H2 (g) → CH4 (g) ΔH=− 74.9kJ H2(g) + 2C(s) + N2 (g) → 2HCN(g) ΔH= + 270.3 kJ
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Use Hess’s law to obtain the enthalpy change for this reaction: H2(g) + 1/8 S8(rhombic) -> H2S(g) from the following enthalpies:H2S(g) + 3/2 O2(g) à H2O(g) + SO2(g) ΔH = -518 KJH2(g) + ½ O2(g) à H2O(g) ΔH = -242 KJ1/8 S8(rhombic) + O2(g) à SO2(g) ΔH = -297 KJ
1) From the following data, C(graphite) + O2(g) à CO2(g) = -393.5 kJ/mol H2(g) + 1/2O2(g) = H2O(l) delta H = -285.8 kJ/mol 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(l) delta H = -3119.6 kJ/mol calculate the enthalpy change for the reaction 2C(graphite) + 3H2(g) =C2H6(g) a) –2417.2 kJ b) –84.6 kJ c) 2417.2 kJ d) –3204.2 kJ