Given the following data: (1) 2 H2(g) + CO2(g) LaTeX: \longrightarrow ⟶ CH4(g) + O2(g) DGorxn...

Question

Question

Given the following data:

(1) 2 H2(g) + CO2(g) LaTeX: \longrightarrow ⟶ CH4(g) + O2(g) DGorxn = 343 KJ

(2) 2 H2(g) + O2(g) LaTeX: \longrightarrow ⟶ 2 H2O(l) DGorxn = -474 KJ

Calculate DGorxn (kJ) for

(3) CH4(g) + 3 O2(g) + 2 H2(g) LaTeX: \longrightarrow ⟶ CO2(g) + 4 H2O(l) DGorxn = ???

Only enter a numerical value.

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Consider the following data. CH4(g) C(s) + 2 H2(g) H = +74.8 kJ C(s) + O2(g) CO2(g) H = -393.5 kJ 2 H2(g) +...

Consider the following data. CH4(g) C(s) + 2 H2(g) H = +74.8 kJ C(s) + O2(g) CO2(g) H = -393.5 kJ 2 H2(g) + O2(g) 2 H2O(l) H = -571.7 kJ Use Hess's law to calculate H for the reaction below. CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l) H = _____ kJ
Given the following data: () 2 H49) + CO (9) CH.(g) + O2(g) AG on =...

Given the following data: () 2 H49) + CO (9) CH.(g) + O2(g) AG on = 343 KJ + 2 H20() AGO -474 KJ (2) 2 H2(g) +049) Calculate AG. (kJ) for – CO(g) + 4 H-00 AG = ??? (3) CH.(g) + 3 O (g) + 2 H (g) Only enter a numerical value. *** please show working and explain **
Given: C6H6(g) + O2(g) LaTeX: \longrightarrow ⟶ CO2(g) + H2O(g) [unbalanced] takes place at 745 mmHg...

Given: C6H6(g) + O2(g) LaTeX: \longrightarrow ⟶ CO2(g) + H2O(g) [unbalanced] takes place at 745 mmHg and 25oC, if 4.00 liters of benzene (C6H6) are consumed in this reaction, how many liters of water can be formed?

Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g)...

Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
Calculate the standard enthalpy of formation of gaseous methane (CH4) using the following thermochemical information: CO2(g)...

Calculate the standard enthalpy of formation of gaseous methane (CH4) using the following thermochemical information: CO2(g) + 2 H2O(l) CH4(g) + 2 O2(g) H = +890.4 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ
Consider the following data. 2 C(s) + H2(g) C2H2(g) H = +226.8 kJ CO2(g) C(s) +...

Consider the following data. 2 C(s) + H2(g) C2H2(g) H = +226.8 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ Use Hess's law to calculate H for the reaction below. 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(l) find kJ

5. Given the following data: (2 H2 (g) + O2 (g) → 2 H2O (1) ro...

5. Given the following data: (2 H2 (g) + O2 (g) → 2 H2O (1) ro in each AH° = -571.6 kJ N20s (g) + H2O (1) 2 HNO3 (1) AH° = -76.6 kJ N2 (g) + 3 O2 (g) + H2 (g) → 2 HNO3 (1) AH° = -348.2 kJ a. Calculate the AHⓇ for the reaction: 2 N2 (g) + 5 O2 (g) → 2 N2O5 (g)
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applica...

Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205
A reaction to produce “substitute natural gas” is described by: 4 CO (g) + 8 H2 (g) → 3 CH4 (g) +...

A reaction to produce “substitute natural gas” is described by: 4 CO (g) + 8 H2 (g) → 3 CH4 (g) + CO2 (g) + 2 H2O (l) Use the following information, as necessary, to estimate DH for the above reaction. 2 C (graphite) + O2 (g) → 2 CO (g)ΔfH= –221.0 kJ/mol 2 CO (g) + O2 (g) → 2 CO2(g)ΔrH= –566.0 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (l)ΔfH= –571.6 kJ/mol C (graphite) + 2...

Given a balance chemical equation, N2(g) + 3 H2(g) LaTeX: \longrightarrow⟶ 2 NH3(g) If a reaction...

Given a balance chemical equation, N2(g) + 3 H2(g) LaTeX: \longrightarrow⟶ 2 NH3(g) If a reaction mixture contains 2 moles of N2(g) and 7 moles of H2(g), which reactant is the limiting reactant and what is the mass (in grams) remaining of the reactant in excess?