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3 years ago

How much heat is required to decompose 25.5 grams of NaHCO3? 2NaHCO3(s) + 129 kJ 2Na2CO3(s) + H2O(

1 answer:

4 0

To determine the heat required in order to decompose a certain amount of a substance, we need information on the heat needed to decompose one mole of the substance. This value are readily available online and other sources. For this reaction, the heat needed is 129 kJ per 2 mol of NaHCO3. We calculate as follows:

129 KJ / 2 mol NaHCO3 (1 mol / 84.01 g ) (25.5 g NaHCO3 ) = 19.58 kJ of heat is needed.

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Consider the model of the nitrogen atom.

liq [111]

Answer:

1s2 2s2 2p3

Explanation:

we know that the number of electrons in an atom is equal to number of protons. So the number of electrons here is 7.

Using Moller chart, the electronic configuration is writen by the electrons first enterring into 1s then into 2s after 2p. The s orbital accomodates maximum of 2 electrons.

∴ for atomic no. 7 nitrogen atom, electronic configuration is 1s2 2s2 2p3.

5 0

3 years ago

Read 2 more answers

The diagram below shows the layers in Earth's interior.

Arada [10]

Answer:

layer B is liquid because of the inner members and layer A is solid because of the outer members

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2 years ago

Insulin is a protein that is used by the body to regulate both carbohydrate and fat metabolism. A bottle contains 525 mL of insu

Mrrafil [7]

Multiply
525 x 40.0 for the total mass (amount) of insulin in the bottle.

Answer: 21,000.0

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7 0

4 years ago

From the enthalpies of reaction H2(g)+F2(g)→2HF(g)ΔH=−537kJ C(s)+2F2(g)→CF4(g)ΔH=−680kJ 2C(s)+2H2(g)→C2H4(g)ΔH=+52.3kJ calculate

DIA [1.3K]

Answer:

$\Delta H$ for the given reaction is -2486.3 kJ

Explanation:

The given equation can be written as a combination of the following equation:

$2H_{2}(g)+2F_{2}(g)\rightarrow 4HF(g)$ ; $\Delta H_{1}= (2\times -537kJ)=-1074 kJ$

$2C(s)+4F_{2}(g)\rightarrow 2CF_{4}(g)$ ; $\Delta H_{2}=(2\times -680kJ)=-1360kJ$

$C_{2}H_{4}(g)\rightarrow 2C(s)+2H_{2}(g)$ ; $\Delta H_{3}=-52.3kJ$

-----------------------------------------------------------------------------------

$C_{2}H_{4}(g)+6F_{2}(g)\rightarrow 2CF_{4}(g)+4HF(g)$

$\Delta H=\Delta H_{1}+\Delta H_{2}+\Delta H_{3}=(-1074-1360-52.3)kJ=-2486.3kJ$

6 0

3 years ago

What would be the volume in liters of an ideal gas, if a 0.425 mole sample of the gas had a temperature of 900 degrees celsius a

Karo-lina-s [1.5K]

The ideal gas law relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a given ideal gas through the equation,

PV = nRT

If we are to determine the volume of the gas, we derive the equation such that it takes the form of,
V = nRT/P

Substituting,
V = (0.425 mol)(0.0821 L.atm/mol.K)(900 + 273 K) / 3 atm

V = 13.64 L

Thus, the volume of the ideal gas is approximately 13.64 L.

5 0

3 years ago