Questions: How many grams of urea are produced from 17.0 g of glycine? Express your answer with the appropriate units.

Solution Steps

The balanced chemical equation for the production of urea from glycine is: \[ \text{2 NH_2CH_2COOH} + \text{O_2} \rightarrow \text{2 NH_2CONH_2} + \text{2 CO_2} + \text{2 H_2O} \]

The molar mass of glycine (NH\(_2\)CH\(_2\)COOH) is: \[ 2(14.01) + 2(1.008) + 2(12.01) + 4(16.00) = 75.07 \, \text{g/mol} \]

The molar mass of urea (NH\(_2\)CONH\(_2\)) is: \[ 2(14.01) + 4(1.008) + 12.01 + 16.00 = 60.06 \, \text{g/mol} \]

Using the molar mass of glycine: \[ \text{moles of glycine} = \frac{17.0 \, \text{g}}{75.07 \, \text{g/mol}} = 0.2264 \, \text{mol} \]

From the balanced equation, 2 moles of glycine produce 2 moles of urea. Therefore, the moles of urea produced are equal to the moles of glycine: \[ \text{moles of urea} = 0.2264 \, \text{mol} \]

Using the molar mass of urea: \[ \text{grams of urea} = 0.2264 \, \text{mol} \times 60.06 \, \text{g/mol} = 13.60 \, \text{g} \]

Final Answer