If everything is under gaseous condition and with equal pressure and temperature, then also 4.0 L SO3 gas is produced from 4.0 L SO2,g.
If 15 liters of propane are completely consumed 90,25 grams of carbon dioxide are produced.
1 mole of sodium carbonate + 2 moles of Hydrochloric acid would produce 1 mole of Carbon Dioxide which would occupy 22.4 liters at standard temperature and pressure
the ratio between HCL and CL2 is 4:2 V(Cl2)=0.98/2=0.49L
The volume of carbon dioxide is 91,9 L at 0 oC.
To determine the number of liters of carbon dioxide produced in this reaction, we need the balanced equation and the molar mass of carbon dioxide. The balanced equation is: CaCO3 + 2HCl → CaCl2 + CO2 + H2O The molar mass of CO2 is 44.01 g/mol. First, we calculate the number of moles of CaCO3: 906 g / molar mass of CaCO3 = moles of CaCO3 Using the balanced equation, we see that the stoichiometric coefficient of CO2 is 1. This means that the number of moles of CO2 produced is equal to the number of moles of CaCO3. Finally, we convert moles of CO2 to liters using the ideal gas law: moles of CO2 x 22.4 L/mol = liters of CO2. Therefore, the number of liters of CO2 produced from 906 grams of CaCO3 can be calculated as follows: liters of CO2 = (906 g / molar mass of CaCO3) x 22.4 L/mol
If 15 liters of propane are completely consumed 90,25 grams of carbon dioxide are produced.
Answer: 68 L NO22NO + O2 ------> 2NO2>68 L + 34 L --> 68 L + some 'left over' NO
88
If I remember chemistry class correctly, it should produce 26.9 L of sulfur dioxide.
The volume of CO2 is 4,94 L.
1 mole of sodium carbonate + 2 moles of Hydrochloric acid would produce 1 mole of Carbon Dioxide which would occupy 22.4 liters at standard temperature and pressure
the ratio between HCL and CL2 is 4:2 V(Cl2)=0.98/2=0.49L
The volume of carbon dioxide is 91,9 L at 0 oC.
7 liters approximately
To determine the number of liters of carbon dioxide produced in this reaction, we need the balanced equation and the molar mass of carbon dioxide. The balanced equation is: CaCO3 + 2HCl → CaCl2 + CO2 + H2O The molar mass of CO2 is 44.01 g/mol. First, we calculate the number of moles of CaCO3: 906 g / molar mass of CaCO3 = moles of CaCO3 Using the balanced equation, we see that the stoichiometric coefficient of CO2 is 1. This means that the number of moles of CO2 produced is equal to the number of moles of CaCO3. Finally, we convert moles of CO2 to liters using the ideal gas law: moles of CO2 x 22.4 L/mol = liters of CO2. Therefore, the number of liters of CO2 produced from 906 grams of CaCO3 can be calculated as follows: liters of CO2 = (906 g / molar mass of CaCO3) x 22.4 L/mol
All one to one here. NaOH + HCl --> NaCl + H2O So, getting the moles of either product tell you how many moles H2O produced. Molarity = moles of solute/Liters of solution moles of solute = Liters of solution * Molarity ( 30.00 mL = 0.03 liters ) Moles H2O = 0.03 Liters * 1 M 0.030 moles H2O produced =================
2.0 billion gallons