### Enthalpy Changes IThe reaction of hydrogen (\( \text{H}_2 \)(g)) with oxygen (\( \text{O}_2 \)(g)) to form water (\( \text{H}_2\text{O} \)(g)) proceeds as follows:\[ 2\text{H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(g) \]When 0.637 g of \( \text{H}_2 \)(g) reacts with sufficient \( \text{O}_2 \)(g), 76.5 kJ is evolved.Calculate the value of \( \Delta H \) for the chemical equation given.\[ \boxed{} \, \text{kJ/mol} \]**Instructions:**1. Fill in the text box with your calculated value of \( \Delta H \).2. Click on "Submit" to check your answer.3. If needed, you can view the approach or detailed steps by selecting "Show Approach" or "Show Tutor Steps".**Note:**You have 4 item attempts remaining.**Options:**- Submit Answer- Try Another Version---

Answered: Image /qna-images/answer/43c3b5ff-54ba-4276-8d74-11513efd130b.jpg

The reaction of hydrogen(g) with oxygen(g) to form water(g) proceeds as follows: 2H2(g) + O2(g)-2H20(g) When 0.637 g H2(g) reacts with sufficient O2(g), 76.5 kJ is evolved. Calculate the value of A,H for the chemical equation given. kJ/mol

The reaction of hydrogen(g) with oxygen(g) to form water(g) proceeds as follows: 2H2(g) + O2(g)-2H20(g) When 0.637 g H2(g) reacts with sufficient O2(g), 76.5 kJ is evolved. Calculate the value of A,H for the chemical equation given. kJ/mol

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...

See similar textbooks

Similar questions

[References] The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3A1(s) +3NH,CIo,(s) → Al,0,(s) + AlCls (s) + 3NO(g) + 6H2O(g) Calculate AH for this reaction. Substance and State AH; (kJ/mol) Al(s) Al2O3 (s) AICI3 (s) H20(g) NO(g) NH CIO.(s) -1676 -704 -242 90. -295 AH: kJ Submit Answer Try Another Version 1 item attempt remaining Prev
The enthalpy of reaction is -11.7 kJ/mol for the following reaction: HCN(aq) + NaOH(aq) --> H2O(l) + NaCN(aq) If 0.541g of HCN react with excess NaOH in a coffee cup calorimeter, what amount will the temperature change by? Use 63.5 g as the total mass in the calorimeter and use 4.184 J/gC as the specific heat. Give your answer to 2 decimal places.
Use the standard reaction enthalpies given below to determine Hᵒrxn for the following reaction: Given: 2 NO(g) + O2(g) → 2 NO2(g) N2(g) + O2(g) → 2 NO(g) 1/2N2(g) + O2(g) → NO2(g) -150. KJ -117 kJ -333 kJ +115 kJ +238 kJ AH°, rxn AHᵒr = ? rxn +183 kJ AH°rxn = +33 kJ
A scientist measures the standard enthalpy change for the following reaction to be -572.6 kJ:H2CO(g) + O2(g)CO2(g) + H2O(l)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(l) is?
The reaction of methane(g) with water(g) to form hydrogen(g) and carbon monoxide(g) proceeds as follows: CH4(g) + H2O(g) -----> 3 H2(g) + CO(g) When 5.41 grams of CH4(g) react with sufficient H2O(g) , 69.5 kJ of energy are absorbed .What is the value of H for the chemical equation given?
Hydrogen cyanide is used in the manufacture of clear plastic such as plexiglas. it is prepared from ammonia and methane according to the following reaction. calculate the value of q(KJ) if 9.436 g of ammonia react with excess oxygen and methane.
a) How would you find the molar enthalpy (in kJ/g) for each fuel and would they compare with each other? b) what are two other factors that can be used to evaluate the fuels
The reaction of ammonia(g) with oxygen(g) to form nitrogen monoxide(g) and water(g) proceeds as follows: 4NH3(g) + 50,(g)–→4NO(g) + 6H2O(g) When 5.96 g NH3(g) reacts with sufficient O2(g), 79.2 kJ is evolved. Calculate the value of A,H for the chemical equation given. kJ/mol
A bomb calorimeter can be used to measure the enthalpy of reaction for combustions, such as the combustion of diborane represented by the following balanced equation: B2H6(g)+3O2(g)=B2O3(s)+3H2O(g)ΔHcombustion for this process is –1958 kJ/mol. Assume that 0.411 g of diborane is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C at 22.61°C. What is the final temperature of the calorimeter?
( is the answer is + 46.48 or -46.48 plzz telll ...why + or why - also explain
According to the reaction below what is the value of KKJ for the complete combustion of 1.00 g of CH4g?
Consider the decomposition of hydrogen bromide to form hydrogen and gaseous bromine, Br2(g): HBr(g) 1/2 H2(g) + 1/2 Br2(g) H = 72.5 kJ (a) What is the enthalpy change for the reverse reaction?Hreverse = _____ kJ/mol(b) Balance the forward reaction with whole-number coefficients. What is H for the reaction represented by this equation?H = _____ kJ/mol