Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- The enthalpy for formation of NH3(g) is -45.9 kJ/mol. What is the reaction enthalpy for the following reaction N2(g)+3 H2(g)+3H2(g)---->2NH3(g)arrow_forwardIn the following reaction, what is the quantity of heat (in kJ) released when 3.91 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO₂ (g) + 2 H₂O(g) AH° = -802 kJ/mol -arrow_forwardThe common fertilizer NH,N0;(s), can explosively decompose according to the following reaction. What is the heat released when 80.06 g of NH,NO;(s) explodes? Molar mass of NH,NO:(s)= 80.06 g/mol. 28. 2 NH,NO3(s) → 2 N2(g) + O2(g)+4 H,O (g) AH = -236.15 kJ -472.3 kJ A) B) -236.15 kJ -118.08 kJ D) -59.04 kJarrow_forward
- A chemist carefully measures the amount of heat needed to raise the temperature of a 1.52 kg sample of C,H,F, from -0.9 °C to 13.0 °C. The experiment 9. 4'2 4 shows that 2.83 × 10" J of heat are needed. What can the chemist report for the molar heat capacity of C,H¸F,? Round your answer to 3 significant digits. - 1 - 1 •K J. mol alo Ararrow_forwardConsider 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 HopHelpCh5N1arrow_forwardIn a popular television series, the two characters use thermite to assist with breaking into a chemical storage facility because the reaction between aluminum and iron(III) oxide produces a tremendous amount of heat. If they began with 10.0 g of Al, how many kJ of heat would be released? 29. 2 Al(s) + Fe,O3(s) → Al,O;(s) + 2 Fe(s) AH = -852 kJ 158 kJ A) B) 236 kJ 472 kJ D) None of the abovearrow_forward
- Determine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g) → 10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g) → AsBr3(g) ΔH = -336.4 kJ/mol As4(s) + 5 O2(g) → As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g) → AsBr5(g) ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g) → Br3AsO(g) ΔH = -295.7 kJ/molarrow_forwardIn a constant-pressure calorimeter, 65.0 mL of 0.910 M H₂SO, was added to 65.0 mL of 0.300 M NaOH. The reaction caused the temperature of the solution to rise from 24.00 °C to 26.04 *C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g °C), respectively), what is AH for this reaction (per mole of H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = V 5 R B 6 MacBook Air N 39 8 M command P option kJ/mol H₂Oarrow_forwardWhat quantity of heat (in kJ) will be released if 0.1673 mol of NH³ are mixed with 0.200 mol of O: in the following chemical reaction? 4 NH (g) + O: (g) → 2 N₂H4 (g) + 2 H₂O (g) AH = -286 kJ/molarrow_forward
- Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. How much heat, in J, was absorbed by the water assuming the specific heat of the water is 4.184 J/g・°C?arrow_forwardIf 10.22 g of a hydrocarbon is combusted inside of a bomb calorimeter with a heat capacity of 722J/C and temperature is raised by 9.5 Chow much heat was lost by the reaction in its combustion?arrow_forward
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