4KO2 + 2H2O+ 4CO24KHCO3 + 3O2
Amount of CO2 exhaled in 5 minutes = Amount of CO2 exhaled per minute X time = 0.702 gram/minute X 5 minute = 3.51 gram
Number of moles of CO2 = amount of the CO2 /mw of CO2 = 3.51 g/44 g/mole= 0.0798 moles
According to the above balanced equation
4 moles of CO2 produces 3 moles of O2
Therefore 0.0798 moles of CO2 will produce = (3/4) X 0.0798 mole O2 = 0.0599 moles O2
Amount of the O2 produced in 5 minutes = number of moles of the O2 produced X mw of O2
= 0.0599 mole X 32 g/mole = 1.91 g. Answer
Oxygen masks for producing O2 in emergency situations contain potassium superoxide, KO2. It reacts with carbon...
Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen: 4KO2 + 2CO2 2K2CO3 + 3O2 This reaction makes potassium superoxide useful in a self-contained breathing apparatus. How much O2 (in grams) could be produced from 2.45 g of KO2 and 4.62 g of CO2?
Potassium superoxide KO2 reacts with carbon dioxide to form potassium carbonate and oxygen 4KO2(s)+2CO2(g)-->2K2CO3(s)+3O2(g) How many moles of O2 will be produced from 2.50 moles KO2 and 1.50 moles of CO2? Please show work using differential analysis
potassium superoxide. KO2 reacts with carbon dioxide, CO2 according to the following equations: 4 KO2 + 2 CO2 --> 2 K2CO3 + 3 O2 When 8 moles of KO2 and 3 moles of CO2 react, the limiting reagent and moles of O2 produced is: KO2 limiting, 6.0 moles O2 CO2 limiting, 12.0 moles O2 KO2 limiting, 3.0 moles O2 CO2 limiting, 4.5 moles O2
Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and nearly quantitative. It is used in submarines, space vehicles, space suits, and by firefighters and miners. 4 KO2(s) + 2 CO2(g) - 2 K2CO3(s) + 3 O2(g) Calculate the mass of KO2 reacted if 355.8 mL of gas is collected over water at 65.0 °C and a barometric pressure of 744.8 torr. (12 pts.) 7. When 12.424 g of (NH4),PO. (FW 149.087 g/mole) is...