1. A piece of sodium metal reacts completely with water as follows: (2Na(s) + 2H_2O(l) ightarrow 2NaOH(aq) + H_2(g)) The hydrogen generated is collected over water at 20°C. The volume of the gas is 260 mL measured at 1.00 atm. Calculate the number of grams of sodium used in the reaction. (Note: assume the vapor pressure of water at 20°C is 0.0363 atm).
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Given: Total pressure = 1.00 atm Partial pressure of water = 0.0363 atm Partial pressure of hydrogen = Total pressure - Partial pressure of water Partial pressure of hydrogen = 1.00 atm - 0.0363 atm Partial pressure of hydrogen = 0.9637 atm Show more…
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Bridger J.
A piece of sodium metal reacts completely with water as follows: $$2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g)$$ The hydrogen gas generated is collected over water at $25.0^{\circ} \mathrm{C}$. The volume of the gas is $246 \mathrm{mL}$ measured at 1.00 atm. Calculate the number of grams of sodium used in the reaction. (Vapor pressure of water at $25^{\circ} \mathrm{C}=0.0313$ atm.
Sodium metal reacts with water to produce hydrogen gas in an exothermic process. $$ 2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g) $$ The reaction was carried out at $25.0^{\circ} \mathrm{C}$ and $760.0 \mathrm{mmHg}$, and the hydrogen gas generated was then collected over water at $23.0^{\circ} \mathrm{C}$ and $785 \mathrm{mmHg}$, yielding $23.1 \mathrm{~L}$ of gas. Calculate the heat evolved; use data from Appendix C.
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