1) 2H2O(g) → 2H2 (g) + O2 (g) DH = 483.6 kJ
If 5 moles of water vapor decompose to form hydrogen and oxygen gas at a pressure of 1.0 atm and 125 oC, what is the change in internal energy of the system?
2)How much heat (in kJ) is evolved when 266 g of white phosphorus (P4 ) burn in air?
P4 (s) + 5O2 (g)---> P4O10(s) DH = -3013 kJ
3) A quantity of 1.00 × 102 mL of 0.500 M HCl was mixed with 1.00 × 102 mL of 0.500 M NaOH in a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solutions was the same, 22.5°C, and the final temperature of the mixed solution was 25.9°C. Calculate the heat change for the neutralization reaction on a molar basis:
NaOH(aq)+HCl(aq)---> NaCl(aq)+H2O(l)
Assume that the densities and specific heats of the solutions are the same as for water (1.00 g/mL and 4.184 J/g·°C, respectively)
4) Choose the thermochemical equation that illustrates ΔH° f for Li2SO4 .
A) 2 Li+ (aq) + SO4 2- (aq) → Li2SO4 (aq)
B) 2 Li(s) + 1/8 S8(s, rhombic) + 2 O2 (g) → Li2SO4 (s)
C) Li2SO4 (aq) → 2 Li+ (aq) + SO4 2- (aq)
D) 8 Li2SO4 (s) → 16 Li(s) + S8(s, rhombic) + 16 O2 (g)
E) 16 Li(s) + S8(s, rhombic) + 16 O2 (g) → 8 Li2SO4 (s) C]
5) Which of the following reactions represents a formation reaction?
5O2 (g) + 2C2H2 (g)→ 2H2O (l) + 4CO2 (g)
CO2 (g) → C (graphite) (s) + O2 (g)
Ca (s) + CO2(g) + ½ O2 (g) → CaCO3(s)
Ca (s) + ½ O2 (g) → CaO (s)
*I want to check over the answers I got for these so if you could show full work/ explanations it would be much appreciated!
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2. Use Hess’s Law to determine the enthalpy of the reaction below. 2F2(g) + 2H2O(l) → 4HF(aq) + O2(g) DH˚= ? H2(g) + F2(g) → 2HF(aq) DH˚ = -546.6 kJ 2H2 (g) + O2(g) → 2H2O(l) DH˚ = -571.6 kJ a. 42 kJ b. -1120 kJ c. -251 kJ d. -521 kJ e. -1690 kJ
1. Consider the following reaction: 2H2(g) + O2(g) → 2H2O(1) ΔH = -572 kJ a. How much heat is evolved for the production of 1.00 mole of H2O(1)? b. How much heat is evolved when 4.03g hydrogen are reacted with excess oxygen? c. How much heat is evolved when 186g oxygen are reacted with excess hydrogen?2. The specific heat capacity of silver is 0.24J/°C g. a. Calculate the energy required to raise the temperature of 150.0g Ag from 273K to 298K. b. Calculate the energy required...
ΔS is negative for the reaction ________. 2H2O (g) → 2H2 (g) + O2 (g) LiOH (aq) → Li+ (aq) + OH– (aq) CH3OH (l) → CH3OH (g) Sr(NO3)2 (aq) + 2LiOH (aq) → Sr(OH)2 (s) + 2LiNO3 (aq) C6H12O6 (s) → 6C (s) + 6H2 (g) + 3O2 (g)
Use the set of three reactions shown below to answer the questions that follow. 2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ 2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ a. If 30.2 g of NO g is reacted with excess oxygen, how much heat energy is produced? b. What mass of liquid water will be consumed during the production of 31000 J of energy assuming that...
Consider the reaction 2H2O(g) →2H2(g) + O2(g) ΔH = +483.60 kJ/mol at a certain temperature. If the increase in volume is 27.7 L against an external pressure of 1.00 atm, calculate ΔU for this reaction. (The conversion factor is 1 L· atm = 101.3 J.) _______kJ
Consider the reaction 2H2O(g) → 2H2(g) + O2(g) ΔH = +483.60 kJ/mol at a certain temperature. If the increase in volume is 42.7 L against an external pressure of 1.00 atm, calculate ΔU for this reaction. (The conversion factor is 1 L · atm = 101.3 J.) _______kJ
4. How many kJ of heat are released when 85.0 g of NaOH reacts with excess H2SO4? H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2 H2O(l) + 114 kJ 5. 2.50 g of octane, CHis was bumed in a bomb calorimeter causing the temperature to increase from 21.0°C to 35.5°C. The total heat capacity of the calorimeter was 8.33 kJ/°C. Calculate the heat of combustion for the reaction shown below. 2 CH 18(1) + 2502(9) ► 16 CO2(g) + 18 H2O(g)...
2. Calculate AH (expressed in kJ/mol) for the following reaction based on the thermochemical information given: Na +Crce → NaCl AH ? Nas) + 2Cl2(g) → Nap + Cle AH = 230 kJ/mol Nag) + Cl → Na(+ Cl® AH = 147 kJ/mol Na(s) + Cl2(e) → NaCl) AH = -411 kJ/mol 3. Consider the reaction: 2HCl) + Ba(OH)2(aq) → BaCl(aq) + 2 H200 AH--118 kJ/mol a. Calculate the heat produced when 700.0 mL of 0.500 M HCl is mixed...
2 pts Question 14 Consider the reaction 2H2(g) + O2(g) → 2H2O(l) AH = -286 kJ Which of the following is true? The reaction is exothermic The reaction is endothermic The reaction is neutral with respect to energy change Heat is absorbed by the system Information is not enough to tell about the energy change
N2H4(l) + O2(g) --> N2(g) + 2H2O (l); LaTeX: \DeltaΔH= -285.8 kJ How many kJ of heat will be released when 14.4 g water is generated? FW: N = 14; H = 1; O = 16. The result should be positive. Keep one digit after decimal.