MP2 Problem Solving

From the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18  +  25O2  --->  16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases.  How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?

Complete the table of reactants and products below and identify the limiting reactant.

Complete combustion of 5.50 g of a hydrocarbon produced 17.7 g of CO, and 6.03 g of H, O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. empirical formula: CH SPECIAL ΔΣΩ λμπ (s) (1) (aq) -> (g) () [ ] -> 1. CLR 3,438 19 SA stv W MacBook Air

Pls help ASAP. Pls make sure to use the GRASS method for both the questions.

Hi! Could you help me with this question? Thank you!

ity College-CHM 101 (Section 90) - Spring20 - MARX > Activities and Due Dates > Ch 7 HW O Assignment Score: O Resources Ly Give Up? 50.1% O Hint Check Answer < Question 16 of 28 The combustion of ethane (C,H.) produces carbon dioxide and steam. 2 C,H,(s) +70,(g) → 4 CO,(g) + 6 H, O(g) How many moles of CO, are produced when 5.05 mol of ethane is burned in an excess of oxygen? moles of CO,: mol terms of use contactus help about us carecrs privacy policy MacBook A

Balance the following chemical equation (ifnecessary):C6H6O(I) + O2(g) -> H20 (g) + CO2 (g)

HAPTER 3 - CHEMICAL REACTIONS Study Page 1 of 3 Next O References Use the References to access important values if needed for this question. hen the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: sulfur (s) + carbon monoxide (g) sulfur dioxide (g) + carbon (s) sp.cengage.info/als-asp/take a 80°F O Type here to search Ca

Chlorination of methane is shown as: Ch4 + Cl2 = CH3Cl + HClIf the feed contains 40% CH4, 50% Cl2 and 10%N2 and 67% of the limiting reactant is converted... What is the composition of methane (in moles) in the product? 11 12 13 14 Composition of chlorine (in moles) in the product? 22 23 24 25

5. Balance the following equation: The combustion of Butane Gas: C4H10  +    O2    --------->        CO2    +    H2O (water) answers are listed in order - 1st coefficient, 2nd coeficient, etc. and so on.     Group of answer choices a) 1,2,2,5 b) 2,6,4,5 c) 2,13,8,10 d) 1,6,4,5

ity 7 Problem-Solving! ctions: Show your solution in the space provided. Follow the GFFSA (Given, Find, omula, Solution, Answer) format if possible. Write your answers in the space provided. (5 points each) 1. Combustion of hydrocarbons like methane (CH4) produces two products, water (H2O) and carbon dioxide (CO2). Consider the chemical equation of this combustlon: CH4 + 2 02- CO2 + 2 H20, when 4 mol of CHa reacts with 4 mol of O2, how many moles of CO2 are formed? What is the limiting reactant? 2. How many grams of lead II chloride are produced from the reaction of 16.2 g of NaCl and 62.0 g of Pb(NO3)27 What is the limiting reactant? How much excess is left over?

Please find the percentage yield from the given info. I have done my best to include everything so that I could ask for help with one thing as I am struggling with finding the percentage yield. if you need to go through the video, please do so. Note: The initial temperature is 128.5 The final temperature is 132.0   Link to the video:  https://drive.google.com/file/d/1BR55ITa7wyOLgLy-MT6ogeXp-fiyuTHn/view?usp=sharing

Q29 Santa Monica Big Blue Bus operates a fleet of CNG buses, which run on compressed natural gas (CNG), natural gas that has been compressed into a much smaller volume in the fuel tank. A newly designed CNG vehicle carries about several thousand cubic feet of compressed natural gas which contain 72 kg (kilograms) of carbon. If all of the natural gas is burned, how many kilograms of carbon dioxide will be emitted into the atmosphere? Assume no residue remains and the carbon dioxide is the only product in the combustion. If you are presenting this question, please explain the following: The steps in the calculation process O Please write out the steps involved in the conversion process including the units O Please explain how to operate on the units Please explain how to manipulate the powers of ten by hand (e.g. product rule and the quotient rule) How to apply the appropriate rule to the calculation: O addition-subtraction rule ("the decimal places rule"), OR multiplication-division…

A nutritional calorie (kcal) is equal to 4.184 kJ. A can of Coca Cola contains 39 g of sugars. We will assume those sugars ultimately all get converted to 39 g of glucose (C6H12O6) in the body. Your body uses glucose in cellular respiration according to the following equation: C6H12O6(s) + 602(g) → 6CO2(g) + 6H₂O (1) a. Using enthalpies of formation provided on the reference page, how many kcal are contained in a can of Coca Cola? You can assume that all the calories in the drink are coming from sugar. b. While carbohydrates (like glucose) and protein provide about 4 nutritional calories per gram consumed, fats (lipids) provide about 9 nutritional calories per gram consumed. What does this tell you about the enthalpy of the reactions that consume fats compared to the enthalpy you determined above for the consumption of glucose?

C = 12.01g /mol H = 1.01g /mol

Q3 The ideal combustion process during which a fuel is burned completely with stoichiometric air is called theoretical (or stoichiometric) combustion. For example, the theoretical combustion of methane is: CH, + a(O, +3.76N,)→6CO, +cH,0+dN, Find the air fuel ratio.