A miner’s lamp burns acetylene (C2H2) that is produced from water dripping onto solid CaC2. The other product formed from the reaction is calcium hydroxide. What volume of water (d = 1.00 g/mL) is required to react with 12.5 g of calcium carbide (CaC2) in the lamp?

calcium bromide + potassium hydroxide ;Balanced chemical equation:Reaction type:

Life support systems of spaceships and submarines are designed assuming that averageconsumption of oxygen for 1 person is 1 kg per day. To obtain oxygen, reaction of sodiumperoxide with carbon dioxide exhaled by people is used (RbO2 + CO2 =>). Calculate the mass of sodium peroxide which must be taken on an expedition to provide oxygen to a crew of 4 people for a week.

Determine the missing pieces in the following reaction. How many liters of gas would be produced from the reaction of 5.5 g aluminum with excess hydrochloric acid? Assume STP conditions. hydrochloric acid (aq) + Al(s) →>> - (aq) +

Write a balanced chemical equation for the standard formation reaction of solid water H2O

The following reaction represents the process known as photosynthesis: 6CO₂(g) + 6H₂O(l) + sunlight → C₆H₁₂O₆(aq) + 6O₂(g). Is photosynthesis a redox reaction? Justify your answer using redox principles.

The town of Andover obtains drinking water from three sources that together produce up to 6.81 × 107 L per day. If effective flocculation requires 9.248 × 10-5 M iron (III) chloride, how many grams of calcium hydroxide are required for treating one day’s worth of water?

The manufacture of nitrogen trifluoride is a growing industry, due to its use as a plasma etchant in the semiconductor industry. Nitrogen trifluoride can be synthesized by passing a current through a high-temperature mixture of ammonium fluoride and hydrogen fluoride, with hydrogen gas as a byproduct. In one synthesis, 1.20x10^3g ammonium fluoride is reacted with1.20x10^3g hydrogen fluoride to produce 5.00x10^2g nitrogen trifluoride. What is the limiting reactant, excess reactant, theoretical yield of nitrogen trifluoride, percent yield, and mass of excess reactant remaining after the reaction?

The Haber Process, developed by Fritz Haber in 1909, was a revolutionary method for producing ammonia from elemental hydrogen and nitrogen on an industrial scale. Write a balanced equation showing the conversion from elemental nitrogen (N2) and hydrogen (H2) to ammonia (NH3). (Omit states-of-matter from your answer.)

4) It takes 62.25 ml of 0.0400 M NazS2O3 solution to completely react with the iodine present in a 175.0 ml iodine solution. How many grams of iodine (12) were initially present in the sample?