2NaOH + H2So4=_____

Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔHrxn = -802.3 kJ.

Olenka [21]

Answer:

1) Minimum mass of methane required to heat 45.0 g of water by 21.0°C is 0.0788 g.

2) Minimum mass of methane required to heat 50.0 g of water by 26.0°C is 0.108 g.

Explanation:

$CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g) ,\Delta H_{rxn} =-802.3 kJ$

1) Minimum mass of methane required to raise the temperature of water by 21.0°C.

Mass of water = m = 45.0 g

Specific heat capacity of water = c = 4.18 J/g°C

Change in temperature of water = ΔT = 21.0°C.

Heat required to raise the temperature of water by 21.0°C = Q

$Q=mc\Delta T= 45.0 g\times 4.18 J/g^oC\times 21.0^oC$

Q = 3,950.1 J = 3.9501 kJ

According to reaction 1 mole of methane on combustion gives 802.3 kJ of heat.

Then 3.950.1 kJ of heat will be given by:

$=\frac{3.950.1 kJ}{802.3 kJ}=0.004923 mol$

Mass of 0.004923 moles of methane :

0.004923 mol × 16 g/mol=0.0788 g

Minimum mass of methane required to heat 45.0 g of water by 21.0°C is 0.0788 g.

2) Minimum mass of methane required to raise the temperature of water by 26.0°C.

Mass of water = m = 50.0 g

Specific heat capacity of water = c = 4.18 J/g°C

Change in temperature of water = ΔT = 26.0°C.

Heat required to raise the temperature of water by 21.0°C = Q

$Q=mc\Delta T= 50.0 g\times 4.18 J/g^oC\times 26.0^oC$

Q = 5,434 J= 5.434 kJ

According to reaction 1 mole of methane on combustion gives 802.3 kJ of heat.

Then 5.434 kJ of heat will be given by:

$=\frac{5.434 kJ}{802.3 kJ}=0.006773 mol$

Mass of 0.006773 moles of methane :

0.006773 mol × 16 g/mol= 0.108 g

Minimum mass of methane required to heat 50.0 g of water by 26.0°C is 0.108 g.

6 0

4 years ago

Classify each statement as a property of ethers, alcohols, or both ethers and alcohols?

natita [175]

Explanation:

1. Only alcohols forms hydrogen bond between themselves and with other compounds containing an O-H, N-H, or F-H bond, such as water.

2. Alcohols up to 4 carbons are miscible in water because they have hydrogen bonded to oxygen and can form hydrogen bond with water. However, it is not possible for ethers.

3. When comparing ethers and alcohols of similar molecular weights, ethers have lower boiling point than alcohol. This is because of the presence of hydrogen bond in alcohols.

8 0

3 years ago

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:

andrezito [222]

Answer: 1.875 moles

Explanation:

2 NaN3(s) → 2 Na(s) + 3 N2(g)

From the equation above, Sodium azide has a chemical formula of NaN3 while nitrogen gas has a chemical formula of N2.

Therefore, If on decomposition

2 moles of NaN3 produce 3 moles of N2

1.25 mol of NaN3 produce Z moles of N2

To get the value of Z, cross multiply

Z x 2 moles = 3 moles x 1.25 moles

2 moles•Z = 3.75 moles²

Divide both sides by 2 moles

2 moles•Z/2 moles = 3.75 moles²/2 moles

Z = 1.875 moles

Thus, 1.875 moles of N2 are produced by the decomposition of 1.25 mol of sodium azide

3 0

4 years ago

Calculate the hydrogen-ion concentration [H+] for the aqueous solution in which [OH-] is 1 x 10-2 mol/L. Is this solution acidid

Lilit [14]

Answer:

[H⁺] = 1.0 x 10⁻¹² M.

Explanation:

[OH⁻] = 1 x 10⁻² mol/L.

∴ [H⁺] = 10⁻¹⁴/[OH⁻] = (10⁻¹⁴)/(1 x 10⁻² mol/L) = 1.0 x 10⁻¹² M.

∵ pH = - log[H⁺] = - log(1.0 x 10⁻¹² M) = 12.0.

∴ The solution is basic, since pH id higher than 7 and also the [OH⁻] > [H⁺].

6 0

4 years ago

In an experiment, 26.5 g of metal was heated to 98.0°c and then quickly transferred to 150.0 g of water in a calorimeter. the in

allsm [11]

This is a common laboratory experiment called calorimetry which determines the specific heat capacity of the sample metal.

By the Conservation of Energy,

Energy of Metal = Energy of Water
mCmetalΔT = mCwaterΔT, wherein Cwater = 4.187 J/g·°C
(26.5 g)(Cmetal)(98 - 32.5°C) = (150 g)(4.187 J/g·°C)(32.5 - 20°C)
Solving for Cmetal,
<em>Cmetal = 4.523 J/g·°C</em>

4 0

3 years ago

2NaOH + H2So4=______+2H2O​

2NaOH + H2So4=______+2H2O