If 1.6 oz of a fuel with a molar mass of 58 g/mol was combusted with a stoichiometric equivalence of oxygen in a mole ratio of 1 mole fuel:4 moles O2. What volume of air would be required? Enter a numerical answer only; do not type the units of L in your answer. Assume the fuel does not affect the concentration of O2 in air. Assumptions: 1 g = 0.03527 oz/;  Air = 28.85 g/mol and 21% O2 (by volume); R=0.082 L.atm/K.mol; T = 298 K

Question 24 of 34 > © Macmillan Learning Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese (IV) oxide. 4 HCl(aq) + MnO₂ (s) → MnCl₂ (aq) + 2 H₂O(l) + Cl₂ (g) A sample of 37.3 g MnO₂ is added to a solution containing 48.9 g HCl. ^ 6 What is the limiting reactant? O MnO₂ OHCI What is the theoretical yield of Cl₂? theoretical yield: If the yield of the reaction is 73.5%, what is the actual yield of chlorine? actual yield: arch or type URL MacBook Pro & 7 * 8 ( 9 0 F + 11 g Cl₂ g Cl₂

Give the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients. C3H8O()+ O₂(g) → CO₂(g) + H₂O() 09 O 5 07 O 10 3

Sodium metal and chlorine gas can be produced by the electrolysis of molten  Sodium chloride as shown in the following equation: 2NaCl(I)-----2Na(I)+ Cl2(g)  What mass of Na in grams would be produced from 10.00 g of NaCl?

For the reaction N, + 3H, 2NH, what is the Mole ratio of nitrogen to hydrogen? t. Mole ratio of hydrogen to ammonia?

2. If 4.9 grams of magnesium metal react with copper (II) bromide to produce 6.2 grams of magnesium bromide and 3.3 grams of copper metal, how many grams of copper (II) bromide were used up? Part II: Balance the following reactions, identify what type of reaction, and Туpе: Redox? write if the reaction is considered a redox reaction. 1 CH, + Oz- 02 CO2+ H20 1) 2._NazSO,+ Pb(NO:)z NaNO, + PbSO. 3. hydrogen gas + oxygen gas - water 3) Liron (III) sulfide + 4. aluminum _aluminum sulfide + iron 4) 2)

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What mass of oxygen is needed for the complete combustion of 6.80×10−3 gg of methane? Express your answer with the appropriate units.

3. You have dissolved 5 g of a rock containing a mixture of calcium carbonate and inert sand in 100 mL of 1 mol L-1 HCI. You measure the calcium concentration of the resulting solution as 0.03 mol L-1 in that 100 mL solution. Calculate the percentage calcium carbonate by weight in the rock sample.

The balanced equation below shows a simple way of manufacturing hydrogen gas in lab (you've done thisl). For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 Al(s) + 6 HCI(aq) -> 2 AICI3(aq) + 3 H2(g) 26.982 36.461 133.341 2.016 What volume of hydrogen gas, in mL, would be produced by the reaction of 922 mg of hydrochloric acid with excess aluminum metal?