Sustainable Energy, Si Edition
2nd Edition
ISBN: 9781337551670
Author: DUNLAP, Richard A.
Publisher: Cengage Learning
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Chapter 3, Problem 10P
To determine
Find the mass of CO and the mass of
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The change in internal energy for the combustion of 1.0 mol of octane at a pressure of 1.0 atm is -5084.3 kJ .
If the change in enthalpy is -5074.0 kJ , how much work is done during the combustion?
Express the work in kilojoules to three significant figures.
Methanol (CH3OH) can be degraded as shown in the reaction below. Answer the following questions if
methanol is present in a water at a concentration of 260 mg/L and the water flowrate is 1.7 million
gallons per day (mgd).
2.
CH3OH + 1.5 O2 → CO2 + 2 HLO
What amount of carbon dioxide (CO2) will be produced each day (in lbs and kg)?
How much oxygen (O2) will need to be supplied to degrade the methanol (in mg/L and lbs/day) if
the oxygen transfer process is 48% efficient?
а.
b.
Given the balanced chemical equation below, what volume of O2 is formed from the decomposition of 13.5 g of HgO if the gas has a pressure of 99 kPa and a temperature of 122°C?
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Sustainable Energy, Si Edition
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- When Ethanol is burn in the presence of Oxygen. Carbon Dioxide (CO2) and water (H2O) molecules are produced. The unbalance reaction of Ethanol and oxygen is given as C2 H5OH + O2→ CO2 +H2O How many grams of Oxygen is required to completely burn 920 grams of Ethanol? Atomic weight: C =12: H = 1: 0 = 16arrow_forward1.Consider the following reaction: CH4 + 2O2 --> 2H2O + CO2 How many moles of water can be formed from 2.4 moles of CH4? 2. Consider the following reaction: 2H 2 + O 2 --> 2H 2O How many moles of water can be formed from 7 mole of H2 and 2.4 moles of O2? 3. How many grams of Fe are produced from 33.2 g of FeO given the following reaction: 3FeO + 2Al --> 3Fe + Al2O3 Be sure to use correct significant figures and units in the answer. 4. For the reaction whose balanced equation is as follows, find how many grams of zinc phosphate will be produced by the reaction of 7.625 grams of zinc chloride. 3 ZnCl2 + 2 (NH4)3PO4 → Zn3(PO4)2 + 6 NH4Cl Be sure to use correct significant figures and units in the answer.arrow_forwardThe combustion of pure hydrogen by the reaction 2H2+O22H2O produces 142 MJ per kg of hydrogen. Compare the energy per kg of octane and the total energy from the individual combustion of its carbon and hydrogen atoms.arrow_forward
- When methanol is used to generate hydrogen, it reacts with the following reaction: CH3OH => CO + 2 H2 The reaction is second order with regards to methanol (CH3OH) and it is observed that 100 g/L of carbon monoxide (CO) can be produced in one day in a batch reactor, if you start with 200 g/L of methanol. What is the rate constant of this reaction (don’t forget to include units)?arrow_forwardA gas undergoes a cycle in a piston-cylinder assembly consisting of the following three processes: Process 1-2: Constant pressure, p = 1.4 bar, V₁ = 0.028 m³, W12 = 10 kJ Process 2-3: Compression with pV = constant, U3 = U₂ Process 3-1: Constant volume, U₁ - U3 = -25 kJ There are no significant changes in kinetic or potential energy. (a) Calculate the net work for the cycle, in kJ. (b) Calculate the heat transfer for process 1-2, in kJ. Part A Your answer is correct. Calculate the net work for the cycle, in kJ. Wcycle = -7.63 kJarrow_forwardThe Bunsen burner in your labs are fueled by natural gas, which is mostly methane, CH4. The thermochemical equations for the combustion of methane (burning in oxygen) is: CH4(g) + 2 O2(g) ➔ CO2(g) + 2 H2O (g) ΔH = – 890.3 kJ/mole Calculate ΔH in kJ when 5.00 g CH4 react with an excess oxygen.arrow_forward
- Cellulose is to be burned in a waste to energy facility. The chemical equation for cellulose is C6H10O5. The atomic weights of C, H, and O are 12, 1, and 16, respectively. The ideal equation for the combustion of cellulose is C6H10O5 +6O2à6CO2 + 5H2O. Calculate the stoichiometric oxygen necessary for the combustion of cellulose. Calculate the stoichiometric air supply. The air is 23.15% oxygen by weight. If the facility operates at 1.5 tons/hour at 100% excess air. How much air is required?arrow_forward2.8. You are given a box containing NH3, N₂, and H₂ at equilibrium at 1000 K. The contents are analyzed, and the following concentrations are found: NH3 = 1.02 mol/L, N₂ = 1.03 mol/L, and H₂ = 1.62 mol/L. Calculate the value of K for the reaction: N2(g) + 3H₂ 2(g) = 2NH₂ ¹3(g)arrow_forwardQ3: B: A 208 g of C6H6 (78 g/mol.) burns in air according to the equation: CHs + O2 - CO2 +H2O What mass of CO2 (44 g/mol.) is produced?arrow_forward
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