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2 years ago

1. The definition of the relative atomic mass for an element, X, is:

Chemistry

1 answer:

sweet-ann [11.9K]2 years ago

7 0

Nolur acil lütfen yalvarırım sana da

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Which of the following statements is true of combustion reactions?

enot [183]

Gasoline contains C and H atoms. During combustion, the carbon (C) from the fuel combines with oxygen (O2) from the air to produce carbon dioxide (CO2).
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O.

Combustion reactions release large amounts of heat. They have negative enthalpy. A negative enthalpy represents an exothermic reaction, releasing heat. This reaction is spontaneous and exothermic, since we can obtain energy from the reaction; the ΔG (free energy) is negative (So 1 is true).

ΔG < 0, so the free energy of the system decreases with the reaction. Remember that when there is a negative ΔG the reaction goes from higher free energy to lower free energy, like in this case.

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2 years ago

Read 2 more answers

how many calories is in one peanut if the volume of water is 10 mL and the water temperature is rise 4 degrees celsius

liraira [26]

Answer:

40.02 calories

Explanation:

V = 10 mL = 10g

we know t went up by 4°C, this is our ∆t as it is a change.

Formula that ties it together: Q = mc∆t

where,

Q = energy absorbed by water

m = mass of water

c = specific heat of water (constant)

∆t = temperature change

Q = (10 g) x (4.186 J/g•°C) x (4°C)

Q = 167.44 J

Joules to Calories:

167.44 J x 1 cal/4.184 J = 40.02 calories

(makes sense as in image it is close to the value).

4 0

2 years ago

Help please

gogolik [260]

Answer:

16 km/2 sec=8km/sec

Explanation:

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2 years ago

Geologists use the Law of Superposition to date rock layers. However, the Earth's

Allisa [31]

The answer is d faults

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2 years ago

Ethanol (C 2H 6O(l), ΔH o f = -277.69 kJ/mol) can be made by reaction of ethylene (C 2H 4(g) ΔH o f = 52.26 kJ/mol) with water (

lidiya [134]

Answer:

Enthalpy change = -44.12 kJ

Explanation:

Given:

ΔH°f(C2H6O(l)) = -277.69 kj/mol

ΔH°f(C2H4(g)) = 52.26 kj/mol

ΔH°f(H2O) = -285.83 kj/mol

To determine:

Enthalpy change for the formation of C2H6O

Calculation:

The given reaction is:

$C2H4(g) + H2O(g)\rightarrow C2H5OH(g)$

The enthalpy change for the reaction is given as;

$\Delta H = \sum n(products)\Delta H^{0}f(products)-\sum n(reactants)\Delta H^{0}f(reactants)$

where n(products) and n(reactants) are the moles of products and reactants

Substituting the appropriate values for n and ΔH°f:

$\Delta H = 1\Delta H^{0}f(C2H6O)-[1\Delta H^{0}f(C2H4)+1\Delta H^{0}f(H2O)]$

ΔH = -277.69-(52.26-285.83) = -44.12 KJ

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3 years ago