A 78.9g sample of HCN contains 0.290g of H and 4.06g of N. Find the mass of carbon in a sample of HCN with a mass of 3.37 g
%H = 0.290/78.9*100 = ?
%N = 4.06/78.9*100 = ?
%C = 100-%H-%N = ?
Then mass C in 3.37 g sample HCN = 3.37 x (%C/100) = ?
To find the mass of carbon in a sample of HCN with a mass of 3.37 g, we need to use the given information about the composition of HCN.
1. Start by subtracting the masses of hydrogen and nitrogen from the total mass of HCN. This will give us the mass of carbon in the sample.
Mass of hydrogen (H) = 0.290 g
Mass of nitrogen (N) = 4.06 g
Total mass of HCN = 3.37 g
Mass of carbon = Total mass of HCN - Mass of hydrogen - Mass of nitrogen
Mass of carbon = 3.37 g - 0.290 g - 4.06 g
2. Calculate the mass of carbon by subtracting the masses:
Mass of carbon = -0.98 g
Since the calculated mass of carbon is negative, it implies that there is an error in the question or the given information is not consistent.
Please double-check the values provided or provide additional information if available.