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
Δ*H* for the reaction, as written.

2 Na(s) + 2 H_{2}O(*l*) → 2 NaOH(*aq*) +
H_{2}(*g*) Δ*H=* ?

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
Δ*H* for the reaction, as written.

2 Na(s) + 2 H_{2}O(*l*) → 2 NaOH(*aq*) +
H_{2}(*g*) Δ*H=* ?

-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

When a 5.93-g sample of solid sodium hydroxide dissolves in 39.8
g of water in a coffee-cup calorimeter (see above figure) the
temperature rises from 22.00 oC to 56.12 oC. Calculate H in kJ/mol
NaOH for the solution process. NaOH(s) Na+(aq) + OH-(aq) The
specific heat of water is 4.18 J/g-K.

Part A
When 2.275 g of anthracene, C14H10, is
combusted in a bomb calorimeter that has a water jacket containing
500.0 g of water, the temperature of the water increases by
43.15°C. Assuming that the specific heat of water is 4.18 J/(g •
°C), and that the heat absorption by the calorimeter is negligible,
estimate the enthalpy of combustion per mole of anthracene.
Part B
The specific heat capacity of methane gas is 2.20 J/g• K. How
many joules of...

Solid sodium reacts violently with water, producing heat,
hydrogen gas, and sodium hydroxide. How many molecules of hydrogen
gas are formed when 48.7 g of sodium are added to water? Write a
balanced equation and then solve.

Aluminum reacts with aqueous sodium hydroxide to produce
hydrogen gas according to the following equation: 2Al(s) +
2NaOH(aq) + 6H2O(l)2NaAl(OH)4(aq) + 3H2(g) The product gas, H2, is
collected over water at a temperature of 20 °C and a pressure of
750 mm Hg. If the wet H2 gas formed occupies a volume of 9.03 L,
the number of grams of H2 formed is g. The vapor pressure of water
is 17.5 mm Hg at 20 °C.

When 4.50 g of Ba(s) is added to 100.00 g of water in a
container open to the atmosphere, the reaction shown below occurs
and the temperature of the resulting solution rises from 22.00°C to
54.35°C. If the specific heat of the solution is 4.18 J/(g • °C),
calculate ΔH for the reaction, as written.
Ba(s) + 2 H2O(l) →
Ba(OH)2(aq) + H2(g) ΔH =
?
When 4.50 g of Ba(s) is added to 100.00 g of water in a...

Aluminum reacts with aqueous sodium hydroxide to produce
hydrogen gas according to the following equation: 2Al(s) +
2NaOH(aq) + 6H2O(ℓ) 2NaAl(OH)4(aq) + 3H2(g) In an experiment, the
H2 gas is collected over water in a vessel where the total pressure
is 758 torr and the temperature is 20°C, at which temperature the
vapor pressure of water is 17.5 torr. Under these conditions, the
partial pressure of H2 is __torr. If the wet H2 gas formed occupies
a volume of 9.60...

Manganese reacts with hydrochloric acid to produce manganese(II)
chloride and hydrogen gas.
Mn(s)+2HCl(aq) →
MnCl2(aq)+H2(g)
When 0.615 g Mn is combined with
enough hydrochloric acid to make 100.0 mL of solution in a
coffee-cup calorimeter, all of the Mn reacts, raising the
temperature of the solution from 24.0 ∘C to 28.4 ∘C.
Find ΔHrxn = ? kJ for the reaction as written. (Assume
that the specific heat capacity of the solution is 4.18 J/g∘C and
the density is 1.00 g/mL.)

Lithium metal reacts with water to produce hydrogen gas and the
corresponding metal hydroxide.
A) Write the balanced chemical equation and describe the type of
reaction
B) How many grams of hydrogen gas will be formed by the complete
reaction of 80.57 g of lithium with water?
C) How many grams of water will be used to produce the hydrogen gas
above?
Please post your work so I can see where I'm going wrong. Thank
you!!

What volume of hydrogen gas is produced when 97.4 g of sodium
reacts completely according to the following reaction at 25 °C and
1 atm?
sodium (s) + water(l)sodium hydroxide (aq) + hydrogen(g)
? liters hydrogen gas

Aluminum metal reacts with hydrochloric acid to produce hydrogen
gas and aluminum chloride (write a balanced equation). When 1.357 g
of Al(s) is combined with 100.0 mL of 3.00M HCl (aq) in a coffee
cup calorimeter, all of the aluminum reacts, raising the
temperature of the solution from 21.5oC to 38.4oC. Find ΔHrxn in
kJ/mol H2. Assume the density of the solution is 1.00 g/mL and the
heat capacity is 4.184 J/goC. Attach a sheet of paper to show your...

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