When a mixture of 10.0 g of acetylene 1C2H22 and 10.0 g ofoxygen 1O22 is ignited, the resulting combustion reactionproduces CO2 and H2O. (a) Write the balanced chemicalequation for this reaction. (b) Which is the limiting reactant?(c) How many grams of C2H2, O2, CO2, and H2O arepresent after the reaction is complete?

If 35g of LiCl mixes with 25g of Ca(OH)2, (a) which is the limiting reactant? (b) what is the theoretical yield? LiCl + Ca(OH)2 → LiOH + CaCl2

Nitrogen (N2)and hydrogen (H2) react to form ammonia(NH3). Consider the mixture of N2 and H2 shown in theaccompanying diagram. The blue spheres represent N, andthe white ones represent H. (a) Write the balanced chemicalequation for the reaction. (b) What is the limiting reactant?(c) How many molecules of ammonia can be made, assumingthe reaction goes to completion, based on the diagram?(d) Are any reactant molecules left over, based on the diagram?If so, how many of which type are left over?

A household water heater containing 50 gallons (227 L) of water is heated burning natural gas (methane, molar mass = 16.043 g mol-1) via the following reaction: CH4(g) + O2(g) CO2(g) + H20(O A,H = -891 kJ mol-1 What mass of methane, in units of g, is needed to heat the 227 L of water in the heater from 25.0°C to 44.0°C? Assume: • the heater is 100% efficient in its use of heat energy • no heat is lost to the surroundings specific heat of water is: 4.184 Jg-1 °C-1 density of water is: 0.9970 g mL¯1

Balance the following chemical equation and determine the number of moles of Fe(s) produced when 1 moles of Fe2O3 (s) react with excess C(s) to produce Fe(s) and CO₂ (g). Fe2O3(s) + C(s) → Fe(s) + CO₂(g)

7.) A Sample Of 13.3g of Fe₂03 reacts with 16.89 CO со to yield Fe and Co₂. The balanced equation Fe₂O3 (s) + 3 C0g 2 Fe (5) + 300₂ (g) is Which Substance is the limiting reactant? What is the theoretical yield of Fe ? If the actual experimental yield for Fe is 8.41g what is the percent yield of Fe?

Ethyl acetate reacts with H2 in the presence of a catalyst to yield ethyl alcohol: C,H,O2(1) + H2(g) → C,H,0(1) (a) Write a balanced equation for the reaction. (b) How many moles of ethyl alcohol are produced by reaction of 1.5 mol of ethyl acetate? (c) How many grams of ethyl alcohol are produced by reaction of 1.5 mol of ethyl acetate with H2? (d) How many grams of ethyl alcohol are produced by reaction of 12.0 g of ethyl acetate with H2? (e) How many grams of H, are needed to react with 12.0 g of ethyl acetate?

(6)For the following balanced reaction use the mass of the chemical provided to solve the mass of the chemical asked for.  6 CO2 +  6 H2O  -->  1 C6H12O6   +   6 O2   202 g of CO2 is consumed by a plant undertaking this photosynthesis reaction.  Find the mass of C6H12O6 produced.

6.24 Ethanol, used in alcoholic beverages, can be produced by the fermentation of sucrose, which is found in sugar cane and other plants. The balanced equation for the fermentation process is C12H„0,(s) + H,0(1) – (a) What mass of ethanol, C,H,OH, would be produced when 2.50 g sucrose reacts by this process? (b) What mass of CO, would also be produced? 4C,H,OH() + 4CO,(g)

1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction.  b) What mass of acetic acid is in the aqueous solution?  c) Which of the reactants is the limiting reagent? Justify your answer.  d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction?  f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?      please answer d, e and f