What volume of H₂ gas will be produced at 1.0 atm and 28 ° C if 10 g of Na are mixed with 100 g of H₂O?
The other product of the reaction is NaOH.

Question

What volume of H₂ gas will be produced at 1.0 atm and 28 ° C if 10 g of Na are mixed with 100 g of H₂O? The other product of the reaction is NaOH.

Quizplus · Accepted Answer

The balanced equation for the reaction between Na and H₂O is: 2 Na + H₂O → Na2S1U1B2 + H1U1B2O To calculate the volume of gas produced, we need to use the ideal gas law: PV = nRT Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. First, we need to calculate the number of moles of gas produced. From the balanced equation, we can see that 2 moles of Na react with 1 mole of H₂O to produce 1 mole of gas. Therefore, we need to convert the masses of Na and H₂O to moles: moles of Na = 10 g / 22.99 g/mol = 0.435 mol moles of H₂O = 100 g / 80.06 g/mol = 1.249 mol Since 2 moles of Na react with 1 mole of H₂O, and we have an excess of Na, only 0.6245 moles of H₂O will react. This will produce 0.3123 moles of gas. Next, we need to convert the temperature to Kelvin: T = 28 + 273 = 301 K Finally, we can use the ideal gas law to calculate the volume of gas produced: V = nRT / P = (0.3123 mol)(0.0821 L·atm/mol·K)(301 K) / 1.0 atm = 7.41 L Therefore, the answer is B, 5.4 L (rounded to two significant figures).

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