Question

A. Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.020 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00°C to 33.60°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written.

2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g) ΔH= ?

Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.020 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00°C to 33.60°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written.

2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g) ΔH= ?

-360 kJ

-90.0 kJ

-180 kJ

-5.41 kJ

B. The specific heat capacity of methane gas is 2.20 J/g• K. How many joules of heat are needed to raise the temperature of 6.00 g of methane from 15.0°C to 36.5°C?

The specific heat capacity of methane gas is 2.20 J/g• K. How many joules of heat are needed to raise the temperature of 6.00 g of methane from 15.0°C to 36.5°C?

680 J

284 J

32.1 J

0.0171 J

58.6 J

Answer 1