32.
Correct option: C
Explanation:
Mass of CO2 produced = 88 g
Molar mass of CO2 = 44 g/mol
Moles of CO2 produced = mass of CO2 produced/molar mass of CO2
= 88 g/44 g
= 2 mol
From the balanced equation given, it is clear that 8 mol of CO2 is produced from 2 mol of butane
Therefore, 2 mol of CO2 is produced from = (2 mol x 2 mol)/8 mol = 0.5 mol of butane.
Molar mass of butane = 58.12 g/mol
Hence, the mass of butane must have reacted = 0.5 mol x 58.12 g/mol = 29 g
13 02 8 Co2 10 H20 If 88 g of carbon dioxide are produced, what mass of butane 2 CAH10 32. must have reacted? D) 58 g C) 29 g A) 116 g B) 14.5 g
The combustion of octane, C, H,, proceeds according to the reaction shown. 18 16 CO,(g)+18 H2O) 2CH18)+2502(g) If 546 mol of octanc combusts, what volume of carbon dioxide is produced at 12.0 "C and 0.995 atm? V = L
Butane, C reacts with Gyoen. O, to form water,H, and carbon dioxide, CO, as shown in the following chemical on: 2CH() +130,($)+10H,O() +SCO,() The coefficients in this equation represent molt s Notice that the coeficient for water (10) is vetimes that of butane (2). Thus the number of moles of water produced is five times the number of moles of butane that react Calculate the mass of water produced when 430g of butane reacts with excess open Express your answer...
2. Ketones have what type of functional group? A) –OH B) C = O C) H – C = 0 D) ----O---- E) COOH 3. Aldehydes have what type of functional group? –OH C=O H-C=O –O— COOH 5. Classify the following reaction: K3P(s) + 2O2(g) --> K3PO4(s) oxidation reduction acid base precipitation 6. Classify the following reaction: K3P(s) + 2O2(g) --> K3PO4(s) oxidation reduction acid base precipitation 7. Classify the following reaction:2KClO3(s) --> 2KCl(s) + 3O2(g) oxidation reduction acid base...
The combustion of octane, C 8 H 18 , proceeds according to the reaction shown. 2 C 8 H 18 ( l ) + 25 O 2 ( g ) ⟶ 16 CO 2 ( g ) + 18 H 2 O ( l ) If 546 mol of octane combusts, what volume of carbon dioxide is produced at 34.0 ∘ C and 0.995 atm?
CH4(g)+O2(g)→CO2(g)+H2O(g) Part A. What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H2O, respectively. Part B. What mass of carbon dioxide is produced from the complete combustion of 8.30×10−3 g of methane? Part C. What mass of water is produced from the complete combustion of 8.30×10−3 g of methane? Part D. What mass of oxygen is needed for the complete combustion of 8.30×10−3 g of...
A major component of gasoline is octane (C₈H₈). When octane is burned in air, it chemically reacts with oxygen gas (O₂) to produce carbon dioxide (CO₂) and water (H₂O) .What mass of carbon dioxide is produced by the reaction of 9.8 g of oxygen gas?
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction of carbon monoxide (CO) with hydrogen (H,). The balanced chemical reaction is: cO@)+2 H, (g)CH,OH() Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen. a. Which reactant is the limiting reagent? b. What is the theoretical yield for methanol? c. At the completion of the reaction, how many grams of the excess reagent will remain? 2. Iron(III) oxide (Fe,O,) can be converted to iron...
A sample of 8.77 g of liquid 1-propanol, C,H, O, is combusted with 40.8 g of oxygen gas. Carbon dioxide and water are the products Write the balanced chemical equation for the reaction. Physical states are optional. chemical reaction: What is the limiting reactant? O oxygen O 1-propanol How many grams of CO, are released in the reaction? mass of CO How many grams of the excess reactant remain after the reaction is complete? mass of excess reactant remaining:
W e applicable 1) Balance the following reaction. _C,H,O + Oai -_CO + H2O a) What mass of O, would be required to react fully with 12.6 g C,H,O?! b) If 5.3 g C,H,O is reacted with 8.85 g 0, identify the limiting reactant. 2) During the lab this week, Magnesium will be reacted with the two acids HCl or H, SO, to produce hydrogen gas and magnesium chloride or magnesium sulfate, respectively. Write out the balanced chemical equations for...