how many liters of carbon dioxide produce when 6kg sodiumcarbonate react with excess hcl at 37 c
Here is a worked example of a stoichiometry problem. Remember, after you found moles CO2 that L = moles x 22.4L/mol at STP. Then convert to other conditions by using the appropriate gas law.
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To determine the number of liters of carbon dioxide produced when 6 kg of sodium carbonate (Na2CO3) reacts with excess hydrochloric acid (HCl) at 37°C, we need to utilize the stoichiometry of the balanced chemical equation.
The balanced chemical equation for this reaction is as follows:
2 Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2
From the balanced equation, we can see that for every 2 moles of Na2CO3, 1 mole of CO2 is produced.
First, we need to calculate the moles of sodium carbonate (Na2CO3) from the given mass of 6 kg. We can do this by utilizing the molar mass of Na2CO3, which is 105.99 g/mol (or 0.10599 kg/mol).
Number of moles of Na2CO3 = mass / molar mass
= 6000 g / 105.99 g/mol
≈ 56.59 mol
Since the stoichiometry of the reaction is 2:1 for Na2CO3 to CO2, the number of moles of CO2 produced would be half of the moles of Na2CO3.
Number of moles of CO2 = 1/2 * moles of Na2CO3
= 1/2 * 56.59 mol
≈ 28.29 mol
Now, to convert the moles of CO2 to liters, we need to use the ideal gas law at the given conditions. The ideal gas law equation is as follows:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
Since the pressure (P) is not provided in the question, we cannot directly calculate the volume (V). However, we can assume the reaction takes place at standard pressure, which is generally taken as 1 atm.
Now let's convert the temperature from Celsius to Kelvin:
37°C + 273.15 = 310.15 K
Using the ideal gas law equation PV = nRT:
V = (nRT) / P
V = (28.29 mol * 0.0821 L·atm/(mol·K) * 310.15 K) / 1 atm
≈ 724.61 L
Therefore, approximately 724.61 liters of carbon dioxide gas would be produced when 6 kg of sodium carbonate reacts with excess hydrochloric acid at 37°C.