The combustion reaction of dimethylhydrazine is used to fuel rockets.
(CH3)2NNH2(l)+4O2(g)N2(g)+4H2O(g)+2CO2(g)
ΔHrxn= –1694 kJ
Calculate the enthalpy change for the following reaction:
2N2(g)+8H2O(g)+4CO2(g)2(CH3)2NNH2(l)+8O2(g)
ΔHrxn= kJ
The combustion reaction of dimethylhydrazine is used to fuel rockets. (CH3)2NNH2(l)+4O2(g)N2(g)+4H2O(g)+2CO2(g) ΔHrxn= –1694 kJ Calculate the...
1st attempt Feedback The combustion reaction of dimethylhydrazine is used to fuel rockets. (CH3)2NNH, (1) +402(8) —— N2(g) + 4H2O(g) +2002(g) AH x = -1694 kJ Calculate the enthalpy change for the following reaction: 2N,(g) + 8H,O(g) + 4CO2(g) → 2(CH3)2NNH, (1) +802 (8) AH - 3388 6 OF 11 QUESTIONS COMPLETED < 05/11 > Bite Balance for olb070 9 Smartwork5 - Goog.
! The combustion reaction of dimethylhydrazine is used to fuel rockets (CH3)2NNH, (1) +40,(8) —— N,(8)+44,0 (8) +200,(8) AH xn = -1694 kJ Calculate the enthalpy change for the following reaction: 2N,(8) +8H20(g) +4C02(8) —> 2(CH3)2NNH, (1) +80, (8) AHxn-
calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187.8 kJ
HQ11.47 Homework. Answered The combustion reaction of nitromethane fuel occurs as follows: 2 CH3 NO2 (1) + 3/2O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g) The standard enthalpy of this reaction is -1418 kJ. What is the standard enthalpy of formation of nitromethane in kJ/mol?
Consider the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔHrxn = -92.6 kJ Calculate the heat (in kJ) given off with the complete reaction of 17.5 grams of hydrogen gas.
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
Consider the two reactions. 2NH3(g)+3N2O(g)4NH3(g)+3O2(g)⟶4N2(g)+3H2O(l)⟶2N2(g)+6H2O(l) Δ?∘=−1010 kJΔ?∘=1531 kJ2NH3(g)+3N2O(g)⟶4N2(g)+3H2O(l) ΔH∘=−1010 kJ4NH3(g)+3O2(g)⟶2N2(g)+6H2O(l) ΔH∘=1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N2(g)+12O2(g)⟶N2O(g)N2(g)+12O2(g)⟶N2O(g)
A.Using standard heats of formation, calculate the standard enthalpy change for the following reaction. N2(g) + 3H2(g) = 2NH3(g) B.Using standard heats of formation, calculate the standard enthalpy change for the following reaction. CaCO3(s) = CaO(s) + CO2(g) C. A scientist measures the standard enthalpy change for the following reaction to be -2910.6 kJ: 2C2H6(g) + 7 O2(g) = 4CO2(g) + 6 H2O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy...
Isobutanol (C4H10O) is anorganic alcohol that is used mainly as a solvent in organic reactions,but can also be used to produce diesel and jet fuel. The first reaction in the manufacturing of diesel isthe production of 2-methylpropene (C4H8): C4H10O(l) ➝C4H8(g) + H2O(g). Use the chemical reactions below to calculate the enthalpy change (ΔHrxn) for the production of 2-methylpropene at 298K.4C(s)+ 5H2(g) + ½O2(g) ®C4H10O(l)DHo= -335 kJ/mol4C(s)+ 4H2(g) ®C4H8(g)DHo= -17 kJ/mol2H2(s)+ O2(g) ®2H2O(g)DHo= -484kJ/mol
The standard enthalpy change for the following reaction is -415 kJ at 298 K. Zn(s) + Ch(g) → ZnCl2() AH° = -415 kJ What is the standard enthalpy change for the reaction at 298 K? ZnCl(s) — Zn(s) + Cl2(g) The standard enthalpy change for the following reaction is -50.6 kJ at 298 K. N2H40 - N2(g) + 2 H2(g) AH° = -50.6 kJ What is the standard enthalpy change for this reaction at 298 K? N2(g) + 2 H2(g)...