Final answer:
607.5 grams of HCL (option C) are needed to completely react with 500.0g of nitrogen monoxide.
To find the grams of HCl needed to react with 500.0g of nitrogen monoxide, calculate the moles of nitrogen monoxide using its molar mass and the grams given. Then use the balanced equation and molar ratio to find the moles and grams of HCl required.
Step-by-step explanation:
To find the grams of HCl needed to completely react with 500.0g of nitrogen monoxide, we need to determine the molar ratio between HCl and nitrogen monoxide. The balanced equation for the reaction is:
2HCl + 2NO → N2O4 + H2O
From the balanced equation, we can see that the molar ratio is 2:2, which means that 2 moles of HCl react with 2 moles of nitrogen monoxide.
Since we know the molar mass of HCl is 36.46g/mol, we can use the molar ratio to calculate the grams of HCl needed.
First, calculate the moles of nitrogen monoxide:
moles of NO = mass of NO / molar mass of NO = 500.0g / 30.01g/mol = 16.66mol
Next, use the molar ratio to find the moles of HCl:
moles of HCl = 16.66mol × (2mol HCl / 2mol NO) = 16.66mol
Finally, calculate the grams of HCl:
grams of HCl = moles of HCl × molar mass of HCl = 16.66mol × 36.46g/mol ≈ 607.5g
Therefore, the answer is 607.5g (option C).