If the combustion of 1.0 mol of CH_4(g) occurs according to CH_4(g) + 2O_2(g) ri

Question

If the combustion of 1.0 mol of CH_4(g) occurs according to CH_4(g) + 2O_2(g) rightarrow CO_2(g) + 2H_2O(l); delta H = -890 kj What is the change in enthalpy for the following reaction? 2 CO_2(g) + 4H_2O(l) rightarrow 2 CH_4(g) + 4O_2(g) From the following reactions with accompanying changes in enthalpy 2H_2(g) + O_2(g) rightarrow 2H_2O(g); delta H = -483.6 KJ 3O_2(g) rightarrow 2 O_3(g); delta H = 284.86 KJ Calculate the heat of reaction for 3 H_2(g) + O_3(g) rightarrow 3 H_2O(g) Experiment #4: An Introduction to Chemical Changes Magnesium metal is added to an aqueous solution of hydrochloric acid. Colorless gas bubbles given off. Write the balanced molecular equation, ionic equation and net ionic equation. For the reaction of aqueous solutions of lead nitrate and potassium iodide give the molecular equation, ionic equation and net ionic equation. Write the chemical reaction for the decomposition of CuSO_4middot 5 H_2O. Experiment #5: The Copper Cycle Write down the Copper Cycle. Which products in the pathway are solids and which are solutions?

Explanation / Answer

2)
reversing the reaction will reverse the sign of delta H
multiplying all the coeeficient by some number will also mutiply delta H by same number

so, delta H new = -2*delta Hold
= -2*(-890 KJ)
= 1780 KJ
Answer: 1780 KJ

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